What volume (in liters) of carbon monoxide gas, measured at a temperature of 212 k and a pressure of 676 mm hg, is required to synthesize 19.3 g of methanol. how many liters of oxygen (at stp) are required to form 12.5 g of h2o ? show your work

For 1: The volume of carbon monoxide required to produce given amount of methanol is 11.9 L.

For 2: The volume of oxygen required to form given amount of water is 7.77 L.

Explanation:

To calculate the number of moles, we use the equation:

    ......(1)

For methanol:

Given mass of methanol = 19.3 g

Molar mass of methanol = 32 g/mol

Putting values in above equation, we get:

The chemical reaction of formation of methanol from carbon monoxide follows:

By Stoichiometry of the reaction:

1 mole of methanol is produced from 1 mole of carbon monoxide.

so, 0.603 moles of methanol will be produced from = of carbon monoxide.

To calculate the volume of carbon monoxide, we use the equation given by ideal gas:

PV = nRT

where,

P = Pressure of carbon monoxide = 676 mmHg

V = Volume of carbon monoxide = ? L

n = Number of moles of carbon monoxide = 0.603 mol

R = Gas constant =

T = Temperature of carbon monoxide = 212 K

Putting values in above equation, we get:

Hence, the volume of carbon monoxide required to produce given amount of methanol is 11.9 L.

Calculating the moles of water by using equation 1, we get:

Given mass of water = 12.5 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

The chemical reaction of formation of water from oxygen and hydrogen follows:

By Stoichiometry of the reaction:

2 moles of water is produced from 1 mole of oxygen gas.

so, 0.694 moles of water will be produced from = of oxygen gas.

At STP:

1 mole of a gas occupies 22.4 L of volume.

So, 0.347 moles of oxygen gas will occupy =

Hence, the volume of oxygen required to form given amount of water is 7.77 L.

c. electrical charges of ionic bonds.