The value of the universal gas constant is 0.082 (L atm)/(mol K) or 8.31 J/(mol k)...

The value of the universal gas constant is 0.082 (L atm)/(mol K) or 8.31 J/(mol k) and 1.00 atm = 760 mmHg or 760 torr.

When a sample of H₂O₂ is decomposed, 350 mL of O₂ gas is collected at 20 °C and at a partial pressure of 695 torr. How many moles of O₂ gas were collect

The value of the universal gas constant is 0.082 (L atm)/(mol K) or 8.31 J/(mol k) and 1.00 atm = 760 mmHg or 760 torr.

Use the balanced equation for the reaction to determine how many grams of H₂O₂ were decomposed in the reaction and how many ml of liquid water would be collected upon cooling (assume a density of water of 1 g/ml)?

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queen_honey_blossom answered 8 months ago

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