How many liters of hydrogen gas is formed from the complete reaction of 15.2 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K .

38 L

Explanation:

There is some info missing. I think this is the original question.

Consider the chemical reaction: C(s) + H₂ O(g) ⟶ CO(g) + H₂ (g). How many liters of hydrogen gas is formed from the complete reaction of 15.2 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K.

Step 1: Write the balanced equation

C(s) + H₂ O(g) ⟶ CO(g) + H₂ (g)

Step 2: Calculate the moles corresponding to 15.2 g of C

The molar mass of C is 12.01 g/mol.

Step 3: Calculate the moles of H₂ produced from 1.27 moles of C

The molar ratio of H₂ to C is 1:1. The moles of H₂ produced are 1/1 × 1.27 mol = 1.27 mol.

Step 4: Calculate the volume of H₂

We will use the ideal gas equation.

2b2t

explanation:

2b2t

35. a insulated cylinder of solid gold (k 310 kw/m-k) of radius v2 m and height 5 m is heated at one end until the temperature at each point in the cylinder is given by w(r, y, z) (30 z2)(2-(r2+ y2). determine the rate of heat flow across each horizontal disk given by z 1, z 2, and z 3, identifying which has the greatest rate of heat flow across it.

explanation: