problem #2: a scientist produces 8.00 moles of water (h2o) using the equation below. how many grams of…

problem #2: a scientist produces 8.00 moles of water (h2o) using the equation below. how many grams of oxygen (o2) were needed? ch4 + 2o2 → co2 + 2h2o 8.00 moles h2o? grams o2 16.0 grams oxygen 64.0 grams oxygen 128 grams oxygen 256 grams oxygen

problem #2: a scientist produces 8.00 moles of water (h2o) using the equation below. how many grams of oxygen (o2) were needed? ch4 + 2o2 → co2 + 2h2o 8.00 moles h2o? grams o2 16.0 grams oxygen 64.0 grams oxygen 128 grams oxygen 256 grams oxygen

Answer

Explanation:

Step1: Determine the mole ratio of (O_2) to (H_2O)

From the balanced chemical equation (CH_4 + 2O_2\rightarrow CO_2 + 2H_2O), the mole ratio of (O_2) to (H_2O) is (2:2 = 1:1).

Step2: Calculate the moles of (O_2)

Given (n(H_2O)=8.00) moles. Since the mole ratio (n(O_2):n(H_2O) = 1:1), then (n(O_2)=8.00) moles.

Step3: Calculate the molar mass of (O_2)

The molar mass of (O) is (16.0) g/mol. For (O_2), (M = 2\times16.0=32.0) g/mol.

Step4: Calculate the mass of (O_2)

Using the formula (m = n\times M), where (n = 8.00) moles and (M = 32.0) g/mol. Then (m=8.00\times32.0 = 256) grams.

Answer:

256 grams oxygen