To solve this we assume that the hydrogen gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant pressure and number of moles of the gas the ratio T/V is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

T1 / V1 = T2 / V2

V2 = T2 x V1 / T1

V2 = (100 + 273.15) K x 2.50 L / (-196 + 273.15) K

V2 = 12.09 L

Therefore, the volume would increase to 12.09 L as the temperature is increased to 100 degrees Celsius.

5 0

4 years ago

If you are using 3.00% (mass/mass) hydrogen peroxide solution and you determine that the mass of solution required to reach the

Maurinko [17]

Answer:

0.004522 moles of hydrogen peroxide molecules are present.

Explanation:

Mass by mass percentage of hydrogen peroxide solution = w/w% = 3%

Mass of the solution , m= 5.125 g

Mass of the hydrogen peroxide = x

$w/w\% = \frac{x}{m}\times 100$

$3\%=\frac{x}{5.125 g}\times 100$

$x=\frac{3\times 5.125 g}{100}=0.15375 g$

Mass of hydregn pervade in the solution = 0.15375 g

Moles of hydregn pervade in the solution :

$=\fraC{ 0.15375 g}{34 g/mol}=0.004522 mol$

0.004522 moles of hydrogen peroxide molecules are present.

5 0

3 years ago

A low-pressure weather system comes into the city of Denver. The atmospheric pressure is 693 mmHg.693 mmHg. If 78.0%78.0% of dry

scoundrel [369]

Answer:

540.54 mmHg

Explanation:

We know that the partial pressure of a substance is defined as; Mole fraction * total pressure.

If the total amount of gases in the atmosphere is 100%, the mole fraction of nitrogen gas is now

78/100 = 0.78

Thus, partial pressure of nitrogen gas = 0.78 * 693 = 540.54 mmHg

6 0

3 years ago