Question

1. if 1.95 moles of h₂o are used, how many grams of co₂ are used?

Explanation:

To solve this, we assume the reaction is the photosynthesis reaction: \(6CO_2 + 6H_2O
ightarrow C_6H_{12}O_6 + 6O_2\) (mole ratio of \(CO_2\) to \(H_2O\) is \(1:1\)).

Step 1: Determine mole ratio

From the reaction \(6CO_2 + 6H_2O
ightarrow C_6H_{12}O_6 + 6O_2\), the mole ratio of \(CO_2\) to \(H_2O\) is \(\frac{n_{CO_2}}{n_{H_2O}}=\frac{6}{6} = 1\). So \(n_{CO_2}=n_{H_2O}\).
Given \(n_{H_2O} = 1.95\) mol, thus \(n_{CO_2}=1.95\) mol.

Step 2: Calculate molar mass of \(CO_2\)

Molar mass of \(C = 12.01\) g/mol, \(O = 16.00\) g/mol.
Molar mass of \(CO_2\), \(M = 12.01 + 2\times16.00=44.01\) g/mol.

Step 3: Calculate mass of \(CO_2\)

Using \(m = n\times M\), where \(n = 1.95\) mol, \(M = 44.01\) g/mol.
\(m = 1.95\space mol\times44.01\space g/mol\approx 85.82\) g.

Answer:

Approximately \(\boldsymbol{85.8}\) grams (or more precisely \(85.82\) grams) of \(CO_2\) are used.