What would be the volume in liters of an ideal gas, if a 0.111 mole sample of the gas had a temperature of 1130 degrees celsius at a pressure of 5.45 atmospheres? (the ideal gas constant is 0.0821 l•atm/mol•k.)

0.43 liters

1.43 liters

1.89 liters

2.35 liters

Option (d) is the correct answer.

Explanation:

The given data is as follows.

      n = 0.111 mole,           T = 1130 degrees Celsius = 1130 + 273 = 1403 K

       P = 5.45 atm,            V = ?

       R = 0.0821 L atm/mol K

Using the ideal gas equation, we can calculate the volume as follows.

                                    PV = nRT

 or,                                V =

                                         =

                                         =

                                         =  2.346 L

or,                                     = 2.35 L (approx)

Thus, we can conclude that volume of the ideal gas is 2.35 liters.

pH = f(x) = -log₁₀x

1. Graphs

I used Excel to calculate the pH values and draw the graphs (see the Figure).

f(x) and f(x) +1 are plotted against the left-hand axis, while f(x+ 1) is plotted against the expanded right-hand axis.

The points at which pH = 0 and pH = 1 are indicated by the large red dots.

2. x = 0.5

When x = 0.5, pH ≈0.30. The point is indicated by the red diamond.

3. Transformations

(a) ƒ(x) = -log(x) + 1

This function has no y-intercept, because log(0) is undefined.

(b) ƒ(x +1) = -log(x + 1)

f(0) = -log(0 + 1) = -log(1) = 0

This function has a y-intercept at (0,0).

hope this helps please mark me brainliest!