Answer:
The Etna volcano when it previously erupted released a lot of smoke, and then volcanic lava.
Explanation:
The eruption of this volcano was on the Italian island of Sicily.
Where there were large columns of smoke and after that the volcanic magma in a viscoelastic state was released into the external environment.
Some sources claim that the eruption of this volcano reached the areas of Zaffanera.
The two products that are formed when a solution of HNO3 and a solution of NaOH react are water and:
NaNO2.
NaNO3.
NaHNO.
NaHNO3.
Answer: NaNO3 (Sodium Trioxonitrate (V) )
Explanation:
The equation of the reaction is; HNO3 + NaOH -----> H2O + NaNO3
Answer: its B
Explanation:
Under what conditions will deviations from the "ideal" gas be expected?
Answer:
Conditions which results in deviating a gas from "ideal" behavior are
1. Low Temperature
2. High Temperature
Explanation:
Ideal gas according to the kinetic model theory states that the conditions that apply are high temperatures where kinetic energy and low pressure is too high and the interactions in between and the container are negligible. Hence, the deviations of ideal gas falls when there is low temperature and high pressure.
What is the average atomic mass of chlorine if 75.8% of chlorine atoms are 35/17 CL with a mass of 34.9589 amu and 24.2% are 37/17 CL with a mass of 36.9659 amu?
Answer:
Explanation:So if a neutron or two is added or removed from the nucleus, then the ... For example Cl–35 has an atomic mass of 35 u (17 protons and 18 neutrons), while Cl–37 ... Calculate the mass contribution of chlorine–35 to the average relative atomic mass ... Which of the following are isotopes of 3517Cl? 1735Cl. 3517Cl. 3717Cl.
Si una masa dada de hidrógeno ocupa 40 litros a 700 grados torr. ¿Qué volumen ocupará a 1 atmósfera de presión? (dar la presión en atmósferas). Por favor :c
Answer:
[tex]V_2=36.84L[/tex]
Explanation:
Hola,
En este caso, podemos usar la ley de Boyle, la cual nos permite analizar el comportamiento volumen-presión en un gas ideal de manera inversamente propocional:
[tex]P_1V_1=P_2V_2[/tex]
Así, dado el volumen y la presión inicial, la cual se convierte a atmósferas (760 torr = 1atm), calculamos el volumen final a 1 atm como se muestra a continuación:
[tex]V_2=\frac{P_1V_1}{P_2}=\frac{700torr*\frac{1atm}{760torr}*40l }{1atm}\\ \\V_2=36.84L[/tex]
Saludos!
Answer:
[tex]V_2=~36.84~Litros[/tex]
Explanation:
En este caso tenemos diferentes valores de volumen y presión para un primer estado:
[tex]V_1=~40~Litros[/tex]
[tex]P_1=~700~torr[/tex]
Y tenemos valores de presión para un segundo estado:
[tex]V_2=~?[/tex]
[tex]P_2=~1~atm[/tex]
Necesitamos una relación entre volumen y presión para poder hallar nuestra incognita ( [tex]V_2[/tex]). Nuestra relación es la ley de Boyle:
[tex]P_1*V_1=P_2*V_2[/tex]
Ahora bien, tenemos una unidad diferente para el presión en [tex]P_2[/tex] (atm), debemos hacer una conversión. Esta conversión puede hacerse si sabemos que 1 atm = 760 torr por lo cual [tex]P_2=760~torr[/tex]
Ahora podemos reemplazar en la ecuación:
[tex]700~torr*40~Litros=760~torr*V_2[/tex]
[tex]V_2=\frac{700~torr*40~Litros}{760~torr}[/tex]
[tex]V_2=~36.84~Litros[/tex]
El volumen sera de 36.84 Litros
Espero que ayude!
What is the mass of 2.13 moles of lithium arsenate
Combustion and corrosion are similar reactions because they both... A) release Carbon Dioxide as a product B) release oxygen as a product C) require oxygen as a reactant D) Have a metal as a reactant
Answer:
B. release oxygen as a product
Explanation:
what is the half-life of the substance as determined by the graph?
Answer:
6.25
Explanation:
Because 2.5 is half and idk know how to explain but yeah
In a titration experiment, a 10.00 ml sample of H2SO4 was titrated with 33.25 mL of 0.777 M KOH.
Calculate (H2SO4).
Answer:
H2SO4 = 0.3885 mol L-1
Explanation:
We need (i) a stoichiometric equation:
H2SO4 + 2NaOH = NaSO4 +2H2O
1:2
And (ii) equivalent quantities of sodium hydroxide
Moles of NaOH = 10x [tex]10^{-3}[/tex]L x 0.777mol [tex]L^{-1}[/tex] = 0.00777 mol
So H2SO4 = (0.5 x 0.00777 mol) / 0.001
= 0.3885 mol L-1
1. What Volume of HCl is generated if 3.44 g of Cl2 are reacted at STP? [tex]H_{2} (g) + Cl_{2}(g) -\ \textgreater \ 2HCl(g)[/tex] 2. What volume does 4.87 mol of Kr have at STP? 3. What pressure of HCl is generated if 3.44 g of Cl2 are reacted in 4.55 L at 455 K?
Answer:
1. 2.17 dm^3
2. 109.1 dm^3
3. 0.398 atm
Explanation:
1. Considering the equation of the reaction;
Number of moles of chlorine gas in 3.44 g= 3.44/2(35.5)= 0.0485 moles
Since we can see from the equation that
1 mole of chlorine gas yields 2(22.4) dm^3 of HCl
0.0485 moles of chlorine gas yields 0.0485 moles × 2(22.4)dm^3/1= 2.17 dm^3
2. Note that 1 mole of Kr occupies 22.4 dm^3
Therefore 4.87 moles of Kr will occupy 4.87 × 22.4 dm^3/1 = 109.1 dm^3
3. From PV= nRT
n= 0.0485 moles
V= 4.55 L
T= 455 K
P= the unknown
R= 0.082 atm dm^3K-1mol-1
P= nRT/V
P= 0.0485 moles × 0.082 atm dm^3K-1mol-1 × 455/4.55
P= 0.398 atm
Answer:
1) volume of HCl = 2.17 L HCl
2) volume of Kr = 109.09 L
3) Pressure of HCl = 0.796 atm
Explanation:
Step 1: Data given
Mass of Cl2 : 3.44 grams
Molar mass Cl2 = 70.9 g/mol
STP = 1atm and 273 K
Step 2: The balanced equation
H2(g) + Cl2(g) → 2HCl(g)
Step 3: Calculate moles of Cl2
Moles Cl2 = mass/ molar mass Cl2
Moles Cl2 = 3.44 grams / 70.9 g/mol
Moles Cl2 = 0.0485 moles
Step 4: Calculate moles HCl
For 1 mol H2 we need 1 mol Cl2 to produce 2 moles HCl
For 0.0485 moles Cl2 we'll have 2*0.0485 = 0.097 moles HCl
Step 5: Calculate volume of HCl
For 1 mol we have 22.4 L
For 0.097 moles we have 22.4 * 0.097 = 2.17 L HCl
Step 1: Data given
Moles of Kr = 4.87 moles
STP = 1 mol, 1atm and 273 K and 22.4 L
Step 2: Calculate volume at STP
1 mol has a volume of 22.4 L
4.87 moles has a volume of 22.4 L * 4.87 = 109.09 L
Step 1: Data given
Mass of Cl2 : 3.44 grams
Molar mass Cl2 = 70.9 g/mol
Volume = 4.55 L
Temperature = 455 K
Step 2: The balanced equation
H2(g) + Cl2(g) → 2HCl(g)
Step 3: Calculate moles of Cl2
Moles Cl2 = mass/ molar mass Cl2
Moles Cl2 = 3.44 grams / 70.9 g/mol
Moles Cl2 = 0.0485 moles
Step 4: Calculate moles HCl
For 1 mol H2 we need 1 mol Cl2 to produce 2 moles HCl
For 0.0485 moles Cl2 we'll have 2*0.0485 = 0.097 moles HCl
Step 5: Calculate pressure of HCl
p*V = n*R*T
⇒with p = the pressure of HCl = TO BE DETERMINED
⇒with V = the volume = the volume of HCl = 4.55 L
⇒with n = the moles of HCl = 0.097 moles
⇒with R = the gas constant = 0.08206 L*atm/mol*K
⇒with T = the temperature = 455 K
p = n*R*T / V
p = (0.097 moles * 0.08206L*atm/mol*K * 455 K) / 4.55 L
p = 0.796 atm
I need help with number 6
(d) greenhouse effect
27. Which event will most likely occur in
rising air?
A. clearing skies
B. cloud formation
C. decreasing relative humidity
D. increasing temperature
Answer:
B. cloud formation
Explanation:
The event that will most likely occur is cloud formation. This is because Rising Air is the key process in the production of clouds and precipitation. This occurs because the air rises and as it rises it begins to expand, it expands so much so that the temperature of the air begins to decrease and humidity rises until cloud droplets begin forming as the excess water vapor condenses on the the air particles.
1. What Volume of HCl is generated if 3.44 g of Cl2 are reacted at STP? 2. What volume does 4.87 mol of Kr have at STP? 3. What pressure of HCl is generated if 3.44 g of Cl2 are reacted in 4.55 L at 455 K?
Answer:
1. 2.17 dm3 VOLUME OF HCl IS PRODUCED WHEN 3.44 g OF Cl2 REACT AT STP
2. 4.87 MOLE OF Kr AT STP CONTAINS 109.088 dm3 .
3. THE PRESSURE WHEN 3.44 g OF Cl2 are reacted at 4.55 L AT 455 K IS 0.77 atm
Explanation:
1 Volume of HCl if 3.44 g of Cl2 are reacted at STP?
Equation for the reaction:
H2 + Cl2 ---------> 2HCl
1 mole of Cl2 reacts to form 2 mole of HCl
At STP, 1 mole of a gas is equal to the molar mass of the gas sample
35.5 * 2 g of Cl2 reacts to form 2 mole of HCl
3.44 g of Cl2 will react to form ( 3.44 * 2 / 71 ) mole of HCl
= 0.0969 mole of HCl
1 mole of HCl = 22.4 dm3
0.0969 mole of HCl = ( 22.4 * 0.0969 / 1)
= 2.17056 dm3
The volume of HCl is 2.17 dm3 when 3.44 g of Cl2 are reacted at STP.
2. What volume does 4.87 mol of Kr have at STP?
1 mole of a substance is 22.4 dm3 of the sample
1 mole of Kr = 22.4 dm3
4.87 mole of Kr = 4.87 * 22.4
= 109.088 dm3
4.87 mole of Kr at STP contains 109.088 dm3 volume
3. Whta pressure of HCl is generated if 3.44 g of Cl2 are reacted at 4.55 L at 455 K
Using the formula:
PV = nRT
V = 4.55 L
R = 0.082 L atm/ mol K
T = 455 K
m = 3.44 g
n = mass / molar mass
molar mass = ( 1 + 35.5) = 36.5 g/mol
n = 3.44 g / 36.5 g/mol
n = 0.094 mole
P = nRT / V
P = 0.094 * 0.082 * 455 / 4.55
P = 3.50714 / 4.55
P = 0.7708 atm
The pressure of HCl if 3.44 g of Cl2 are reacted at 4.55 L and 455 K is 0.7708 atm.
1. The volume of HCl generated is 2.15 L
2. The volume of 4.87 moles of Kr is 109.088 L
3. The pressure of HCl generated is 0.788 atm
1. Determination of the volume of HCl generated
We'll begin by calculating the number of mole in 3.44 g of Cl₂Mass of Cl₂ = 3.44 g
Molar mass of Cl₂ = 2 × 35.5 = 71 g/mol
Mole of Cl₂ =?Mole = mass / molar mass
Mole of Cl₂ = 3.44 / 71
Mole of Cl₂ = 0.048 mole Next, we shall determine the mole of HCl produced.H₂ + Cl₂ —> 2HCl
From the balanced equation above,
1 mole of Cl₂ reacted to produce 2 moles of HCl.
Therefore,
0.048 mole of Cl₂ will react to produce = 0.048 × 2 = 0.096 mole of HCl
Finally, we shall determine the volume of HCl generated at STP.At standard temperature and pressure (STP),
1 mole of HCl = 22.4 L
Therefore,
0.096 mole of HCl = 0.096 × 22.4 = 2.15 L
Thus, the volume of HCl generated at STP is 2.15 L
2. Determination of the volume of 4 moles of Kr at STP
At standard temperature and pressure (STP),
1 mole of Kr = 22.4 L
Therefore,
4.87 moles of Kr = 4.87 × 22.4 = 109.088 L
Thus, 4.87 moles of Kr has a volume of 109.088 L at STP
3. Determination of the pressure of HCl generated.
Number of mole (n) of HCl obtained = 0.096 mole
Volume (V) = 4.55 L
Temperature (T) = 455 K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure (P) =?
PV = nRT
P × 4.55 = 0.096 × 0.0821 × 455
P × 4.55 = 3.586128
Divide both side by 4.55
P = 3.586128 / 4.55
P = 0.788 atmThus, the of HCl generated is 0.788 atm
Learn more: https://brainly.com/question/16897574
describe a change caused by kenitic energy as well as a change that involves potential energy
Photochemical smog consists of a) coal dust b)water droplets and soot c) ozone d) acid rain
Answer:
the answer is C Ozone
hope that helps
The minimum amount of unstable atoms needed to produce an uncontrolled chain reaction is called _____.
atomic mass
mass number
critical mass
balance each equation by entering the correct coefficients.
Answer:
5SiO2 + 2CaC2 --> 5Si + 2CaO + 4CO2
4NH3 + 5O2 --> 4NO + 6H2O
Q2: A compound consists of 40.00 % C, 6.67 % H and
rest is oxygen by mass. If RMM of X is 180, find the
molecular formula.
Answer:
C6H12O6
Explanation:
Just use the table method like I did and compared the molecular mass with the mass of the empirical formula.
If I dilute 120 mL of a 1.3 M solution until the new concentration is 0.83 M, what is the new volume? Round to the nearest WHOLE NUMBER and DO NOT include units. *
1 point
Answer:
[tex]V_2=188mL[/tex]
Explanation:
Hello,
In this case, for dilution processes, the initial moles must be the same to the final moles, therefore, only the volumes and molarities change from the beginning to the end of the dilution:
[tex]M_1V_1=M_2V_2[/tex]
In this case, we are asked to compute the new or final volume, so we simply solve for it as shown below:
[tex]V_2=\frac{M_1V_1}{M_2}=\frac{120mL*1.3M}{0.83M}\\ \\V_2=188mL[/tex]
Best regards.
I AM GIVING BRAINLIEST! PLEASEEEEEE HELPPPPPP I NEED HELPPP
How many atoms of nitrogen in 2.0 mol of dinitrogen monoxide, N2O?
Answer:
I think that the answer is N20:2(14.01)+1(16.06)=44.02g/mol(c) fluorine Di nitrogen monoxide contains how many mom 6.022 x
1023 mol N20
Which type of burn injury can convert to a deeper injury due to tissue hypoxia?
Answer:
Deep partial-thickness wounds
How many atoms are contained in 97.6 g of platinum (Pt)?
Answer:
3.01 * 10 ^ 23 atoms of Pt
Explanation:
1 mole of Pt contains 6.02 * 10 ^ 23 atoms of Pt
195.084 g of Pt has 6.02 * 10 ^ 23 atoms of Pt
97.6 g = .5 moles so
97.6 g of Pt has 3.01 * 10 ^ 23 atoms of Pt
The 97.6 grams of platinum contains [tex]3.011\times 10^{23}[/tex] atoms.
Given:
The mass of platinum = 97.6 grams
To find:
The number of platinum atoms in 97.6 grams.
Solution:
Mass of platinum = 97.6 g
Moles of platinum =[tex]\frac{97.6g}{195.084 g/mol}=0.500 mol[/tex]
According to the mole concept:
1 mole = Avogadro Number = [tex]N_A=[/tex] [tex]6.022\times 10^{23} atoms/ molecules/ions[/tex]
The number of platinum atoms in 0.500 moles of platinum:
[tex]=0.500\times 6.022\times 10^{23} atoms\\\\=3.011\times 10^{23} atoms[/tex]
The 97.6 grams of platinum contains [tex]3.011\times 10^{23}[/tex] atoms.
Learn more about the mole concept here:
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Blood rich in carbon dioxide was called venous blood, as it was believed that only the veins carried this type of blood. Based on what you know about the circulatory system, explain why this statement is incorrect.
Answer:
Yes is incorrect
Explanation:
not all veins carry blood rich in CO2 , the pulmonary vein carries blood with O2 which means that not all veins carry blood rich in CO2
What volume of 0.500 M HNO₃(aq) must completely react to neutralize 100.0 milliliters of 0.100 M KOH(aq)?
Answer:
v = 500 milliliters
Explanation:
[tex]HNO_{3}[/tex] ⇒ [tex]H^{+} + NO^{3-}[/tex]
[tex]KOH[/tex] ⇒ [tex]K^{+} + OH^{-}[/tex]
1 [tex]H^{+}[/tex] to 1 [tex]OH^{-}[/tex]
[tex]\frac{0,5}{V} = \frac{0,1}{100} \\\\v * 0,1 = 50\\v = 500 milliliters[/tex]
how many liters of hydrogen gas is produced from 3.712 g of magnesium with 104.2ml of 1.385 mol/L HCL (aq) at SATP?
Please help me!! I need to figure this question out for a quiz.
Answer:
The correct answer is 1.61 L.
Explanation:
Based on the given information, 3.712 grams of Mg reacts with 104.2 ml of 1.385 mol per L HCl at SATP, there is a need to find the amount of hydrogen gas produced in liters.
The chemical reaction taking place in the given case is,
Mg + 2HCl = MgCl2 + H2
The reacting moles of each reactants is,
Moles of Mg = 3.712 g/24.305 g = 0.153 moles
Moles of HCl = 1.385 mol/L * 0.1042 L = 0.144 moles
From the reaction it is clear that Mg and HCl are present in 1:2 molar ratio. Therefore, 0.153 moles of Mg can completely react with 0.306 moles of HCl. However, the moles of HCl obtained in the given case is only 0.144 moles, thus, HCl is a limiting reactant.
Now the moles of hydrogen produced is,
n = 0.144 moles of HCl * (1 mole H2/2 mol HCl) = 0.072 moles
Finally to find the liters of hydrogen gas produced, the ideal gas equation is used, that is, PV = nRT
At STAP, the value of T is 273 K and pressure is 1 atm, the value of R is 0.082 atm.L/mol.L. Now putting the values we get,
PV = nRT
V = nRT/P
V = 0.072 mol * 0.082 atm.L/mol.L*273/ 1 atm
V = 1.61 L
please at least answer one! Determine the formula mass of each of the substances below.
1. CaCl2
2. NH4OH
3. AgCH3COO
4. Ba3(PO4)2
5. Al2(CO3)3
6. Zn(NO3)2
Someone please help! I've been stuck on this for hours :(
Answer:
Explanation:
1. 40.08 + 35.45(2) = 110.98
2. 14.01 + 1.01(5) + 16.00 = 35.06
3. 107.87 + 12.01(2) + 1.01(3) + 16.00(2) = 165.91
4. 137.33(3) + 30.97(2) + 16.00(8) = 601.93
5. 26.98(2) + 16.00(9) + 12.01(3) = 216.06
6. 65.39 + 14.01(2) + 16.00(6) = 189.41
Check me if I'm wrong.
What is the total mass of Kr-42 remaining in a 20-mg sample after 48.8 hours?
(1) 2.5 mg
(2) 5.0 mg
(3) 10 mg
4) 20 mg
Answer:
2.5milligram
Explanation:
Due to Kr-42 the 20mg will diluted to the experinental evluation
Which of the following is NOT a true state-
ment about gases?
Answer:
Unsure there's not enough information to answer
Explanation:
Which of the following is NOT a true statement about gases?
how do shinny pots or pans reflect light
Answer:
Yes they do
Explanation:
This is because the light that shines on the pots and pans reflect back considering that they are shinny.
Answer:
Polished shiny surfaces reflect light because they have a even surface.
Explanation:
The polished shiny surfaces being smooth and lustrous, absorb very little amount of light and reflect more.
Pls Brainliest!!
What is
ground water?
Answer:
Water that is present beneath the Earth's surface
Please help!!
How many moles of sodium carbonate (Na2CO3) are required to precipitate the calcium ion from 803.1 mL of a 0.35 M CaCl2 solution?
Answer:
[tex]n_{Na_2CO_3}=0.28molNa_2CO_3[/tex]
Explanation:
Hello,
In this case, the undergoing chemical reaction is:
[tex]Na_2CO_3(aq)+CaCl_2(aq)\rightarrow CaCO_3(aq)+2NaCl(aq)[/tex]
Hence, given the solution of calcium chloride, we can compute its reacting moles:
[tex]n_{CaCl_2}=0.35\frac{mol}{L}*803.1mL*\frac{1L}{1000mL}= 0.28molCaCl_2[/tex]
Thus, by knowing there is a 1:1 molar ratio between sodium carbonate and calcium chloride, we can easily compute the moles of sodium carbonate needed for a complete precipitation as shown below:
[tex]n_{Na_2CO_3}=0.28molCaCl_2*\frac{1molNa_2CO_3}{1molCaCl_2} \\\\n_{Na_2CO_3}=0.28molNa_2CO_3[/tex]
Best regards.