All categories

4 years ago

A 500. mL gas sample is collected over water at a pressure of 740 mmHg and 25.0 °C. What is the volume of the dry gas at STP?

Chemistry

1 answer:

Lera25 [3.4K]4 years ago

7 0

Answer:

Volume of dry gas at STP = 0.432 liters or 432 ml

Explanation:

Given:

Pressure (P) = 740 mmHg - 24 mmHg = 716 mmHg

Temperature (t) = 25 degrees C + 273 K = 298 K

500 ml = 0.5 l

Find:

Volume of dry gas at STP

Computation:

[P1][V1] / T1 = [P2][V2] / T2

[716][0.5] / 298 K = [760][ x Liters] / 273 K

x = 0.432 Liters

Volume of dry gas at STP = 0.432 liters or 432 ml

You might be interested in

State whether the following statements are true or false (with justification). (a) 1 mol of N2 has more molecules than 1 mol of

MAVERICK [17]

Answer:

A. False.

Every substance contains the same number of molecules i.e 6.02x10^23 molecules

B. False.

Mass conc. = number mole x molar Mass

Mass conc. of 1mole of N2 = 1 x 28 = 28g

Mass conc. of 1mol of Ar = 1 x 40 = 40g

The mass of 1mole of Ar is greater than the mass of 1mole of N2

C. False.

Molar Mass of N2 = 2x14 = 28g/mol

Molar Mass of Ar = 40g/mol

The molar mass of Ar is greater than that of N2.

Explanation:

7 0

3 years ago

Calculate the pH of a solution that is 0.147M HCl

Mariana [72]

Answer:

pH = 0.832

Explanation:

pH is given by the formula;

pH = - log [H+]

in this case we are given 0.147 M HCl

HCl is a strong acid and therefore completely dissociates to give out H+ ions,

Therefore; [H+] = [HCl] = 0.147 M

Hence;

pH = - log 0.147 M

3 0

3 years ago

The compound borazine consists of 40.29% boron, 7.51%

ioda

Answer:

$B_3H_6N_3$

Explanation:

Hello there!

In this case, since the mass percentages in a compound which is wanted to know the molecular formula, can be assumed to be the masses, we first need to compute the moles they have in the formula unit:

$n_B=40.29gB*\frac{1molB}{10.811gB} =3.73molB\\\\n_H=7.51gH*\frac{1molH}{1.01gH} =7.44molH\\\\n_N=52.20gN*\frac{1molN}{14.01gN} =3.73molN$

Next, we divide each moles by the fewest ones (3.73 mol) in order to find the subscript in the empirical formula first:

$B:\frac{3.73}{3.73}=1 \\\\H:\frac{7.44}{3.73}=2\\\\N:\frac{3.73}{3.73}=1$

Then, the empirical formula is BH2N whose molar mass is 26.83 g/mol, so the ratio of molecular to empirical is 80.50/26.83=3; therefore, the molecular formula is three times the empirical one:

$B_3H_6N_3$

Best regards!

7 0

3 years ago

Titanium dioxide (TiO ) is used extensively as a white pigment. It is produced from an ore that contains ilmenite (FeTiO ) and f

rusak2 [61]

Answer:

= 7392 kg solution

Explanation:

detailed solving is given in the attached document.