.How many moles of O2(g) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO2(g) and H2O(g) according to the following reaction: CH4(g) + 2O2  CO2(g) + 2H2O(g)

4.64 moles of O₂ are needed.

Explanation:

Determine the balance reaction:

CH₄(g) +  2O₂(g)  →  CO₂(g)  +  2H₂O(g)

We verify the amount of methane at STP by the Ideal Gases Law

P . V= n . R . T

STP → 1 atm of pressure, 273K of T° (Standard conditions)

1 atm . 52L = n . 0.082 . 273K

(1 atm . 52L) / (0.082 . 273K) = n

52 / (0.082 . 273K) = n → 2.32 moles of CH₄

1 mol of methane reacts with 2 moles of oxygen

Then, 2.32 moles of methane must react with 4.64 moles of O₂ (2.32 .2) /1

coral.

explanation:

coral. many marine organisms that produce calcium carbonate shells or skeletons are negatively impacted by increasing co2 levels and decreasing ph in seawater.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation: