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zalisa [80]
3 years ago
15

A 8.5 L sample is collected at 45°C. What will the volume be if the temperature is raised to 70°C? End of exam A. 9.2 L B. 13.2

L C. 7.9 L D. 5.5 L
Chemistry
1 answer:
klasskru [66]3 years ago
7 0

Answer: The correct option is A.

Explanation: To calculate the volume at the end , we use Charles's Law, which states that the volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

V\propto T

or

\frac{V_1}{T_1}=\frac{V_2}{T_2}

  • Initial conditions:

V_1=8.5L

T_1=45^oC=(45+273)K=318K

  • Final conditions:

V_2=?L

T_2=70^oC=(70+273)K=343K

Putting all the values in above equation, we get

\frac{8.5}{318}=\frac{V_2}{343}

V_2=9.2L

Hence, the correct option is A.

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How does shaking or stirring a mixture of solute and solvent affect a solution?
MA_775_DIABLO [31]
I know this one it’s B
3 0
3 years ago
A sample of gas has a mass of 38.8 mg. Its volume is 224 mL at a temperature of 55 °C and a pressure of 886 torr. Find the molar
Pie

Answer:

4g/mol

Explanation:

Firstly, we can get the number of moles of the gas present using the ideal gas equation.

PV = nRT

Here:

P = 886 torr

V = 224ml = 224/1000 = 0.224L

T = 55 degrees celcius= 55+ 273.15 = 328.15K

R = molar gas constant = 62.36 L⋅Torr⋅K−1⋅mol−1

n = PV/RT

n = (886 * 0.224)/(62.36 * 328.15)

n = 0.009698469964 mole

Now to get the molar mass, this is mathematically equal to the mass divided by the number of moles. We have the mass and the number of moles, remaining only the molar mass.

First, we convert the mass to g and that is 38.8/1000 = 0.0388

The molar mass is thus 0.0388/0.009698469964 = 4g/mol

3 0
4 years ago
How many moles of nitrous oxide (N2O) are produced when 1.40 moles of ammonium nitrate (NH4NO3) decompes?
blagie [28]

Answer:

The answer to your question is 1.40 moles of N₂O

Explanation:

Balanced equation

                           NH₄NO₃   ⇒   N₂O  +  2 H₂O

                                 2   --------   N  ---------- 2

                                 4   -------    H  ---------- 4

                                 3   -------    O  ---------- 3

Process

1.- From the balanced equation, we know that 1 mol of NH₄NO₃ produces 1 mol of N₂O so, we use proportions to find the number of moles produced when 1.40 moles of NH₄NO₃ react.

                           1 mol of NH₄NO₃  ------------- 1 mol of N₂O

                           1.40 moles            --------------   x

                           x = (1.40 x 1) / 1

                            x = 1.40 moles of N₂O are produced

7 0
4 years ago
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