What is the molar mass of a gas whose density at stp is 3.74 g/l?
1 answer:
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<em>Calculate the pH of the following substances formed during a volcanic eruption: </em>
<em>• Acid rain if the [H +] is 1.9 x 10-5 </em>
<em>• Sulfurous acid if [H +] = 0.10 </em>
<em>• Nitric acid if [H +] = 0.11</em>
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<h3>Further explanation </h3>pH is the degree of acidity of a solution that depends on the concentration of H⁺ ions. The greater the value the more acidic the solution and the smaller the pH.
pH = - log [H⁺]
- pH acid rain
- pH Sulfurous acid
- pH Nitric acid
<u>Answer:</u> The amount of water that can be formed is 160 moles
<u>Explanation:</u>
We are given:
Moles of hydrogen gas = 170 moles
Moles of oxygen gas = 80 moles
The chemical equation for the reaction of hydrogen gas and oxygen gas follows:
By Stoichiometry of the reaction:
1 mole of oxygen gas reacts with 2 moles of hydrogen gas
So, 80 moles of oxygen gas will react with = of hydrogen gas
As, given amount of hydrogen gas is more than the required amount. So, it is considered as an excess reagent.
Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of oxygen gas produces 2 moles of water
So, 80 moles of oxygen gas will produce = of water
Hence, the amount of water that can be formed is 160 moles