What volume of Cl2 gas, measured at 687 torr and 39 C, is required to form 23 g

Question

What volume of Cl2 gas, measured at 687 torr and 39 C, is required to form 23 g of NaCl? Express your answer using two significant figures.

A sample of gas in a balloon has an initial temperature of 20. C and a volume of 1.67×103 L . If the temperature changes to 71 C , and there is no change of pressure or amount of gas, what is the new volume, V2, of the gas?

Express your answer with the appropriate units.

What Celsius temperature, T2, is required to change the volume of the gas sample in Part A (T1 = 20. C , V1= 1.67×103 L ) to a volume of 3.34×103 L ? Assume no change in pressure or the amount of gas in the balloon.

Express your answer with the appropriate units.

Explanation / Answer

1)

moles of NaCl = 23 / 58.5 = 0.393

2 Na + Cl2 ----------> 2 NaCl

1 mol Cl2   --------------> 2 mol NaCl

   ??          -----------------> 0.393 mol NaCl

moles of Cl2 gas = 0.1966 mol

pressure = 687 torr = 0.9039 atm

temperature = 39 + 273 = 312 K

P V = n R T

0.9039 x V = 0.1966 x 0.0821 x 312

V = 5.57 L

volume of Cl2 gas = 5.57 L

2)

temperature T1 = 20 + 273 = 293 K

volume V1 = 1.67×103 L

temperature T2 = 344 K

volume V2 = ??

V1 / T1 = V2 / T2

1.67×103 / 293 = V2 / 344

V2 = 1.96 x 10^3 L

new volume = 1.96 x 10^3 L

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