All categories

3 years ago

The volume of a gas is 17.5 mL at 29◦C and

Chemistry

1 answer:

mars1129 [50]3 years ago

8 0

Answer: V = 14.4 mL

Explanation:

In this case, we'll use the ideal gas formula:

PV = nRT

Where:

P: pressure in atm

V: volume in liter

n: moles

R: gas constant (In this case 0.082 L atm/mol K)

T: temperature in K

We have data for the gas at first, so we can actually calculate the moles used, which will be constant even at different temperature and pressure. Let's calculate the moles:

n = PV/RT

Before we do this, let's convert the volume and temperature:

T = 29 + 273 = 302 K

V = 17.5 / 1000 = 0.0175 L

Now the moles:

n = 0.863 * 0.0175 / 0.082 * 302 = 0.00061 moles

with these moles, let's convert the temperature to K:

T2 = 13 + 273 = 286 K

and to calculate the volume:

V = nRT/P

so:

V = 0.00061 * 0.082 * 286 / 0.994

V = 0.0144 L or simply 14.4 mL

You might be interested in

How many σ and π bonds are present in a molecule of cumulene?

dimaraw [331]

A hydrocarbon with three or more consecutive (cumulative) double bonds is known as a cumulene. They are analogous to allenes, only exhibiting a more elongated chain. The basic molecule in this category is butatriene, which is also simply known as cumulene.

In the structure of a cumulene, there are 3 double bonds and 4 single bonds. The double bond comprises 1 sigma bond, and 1 pi bond and 4 hydrogen bond produces a sigma bond with carbon. Thus, the molecule of cumulene comprises 7 sigma bonds and 3 pi bonds.

3 0

3 years ago

Read 2 more answers

The equilibrium constant, Kc, for the following reaction is 0.967 at 650 K. 2NH3(g) N2(g) 3H2(g) When a sufficiently large sampl

AlekseyPX

Answer: Concentration of $NH_3$ in the equilibrium mixture is 0.31 M

Explanation:

Equilibrium concentration of $H_2$ = 0.729 M

The given balanced equilibrium reaction is,

$2NH_3(g)\rightleftharpoons N_2(g)+3H_2(g)$

Initial conc. x 0 0

At eqm. conc. (x-2y) M (y) M (3y) M

The expression for equilibrium constant for this reaction will be:

3y = 0.729 M

y = 0.243 M

$K_c=\frac{[y]\times [3y]^3}{[x-2y]^2}$

Now put all the given values in this expression, we get :

$K_c=\frac{0.243\times (0.729)^3}{(x-2\times 0.243)^2}$

$0.967=\frac{0.243\times (0.729)^3}{(x-2\times 0.243)^2}$

$x=0.80$

concentration of $NH_3$ in the equilibrium mixture = $0.80-2\times 0.243=0.31$

Thus concentration of $NH_3$ in the equilibrium mixture is 0.31 M

3 0

3 years ago

Use the portion of the periodic table shown below to answer the questions.

Basile [38]

Part 1: Potassium, and Rubidium.
Part 2: Calcium has 20 protons and 20 electrons because the atomic number for calcium is 20 and that determines how many protons there are and in an atom, the number of protons is the same number of electrons. Calcium has about 20 neutrons. I got the number of Neutrons by subtracting the mass number(40.078) and the atomic number(20), I got 20.078. Round to the nearest whole number because you cannot have half or partial neutron. So, Calcium has 20 protons, 20 electrons, and 20 neutrons,

Hope this helps and please mark as brainliest!

8 0

4 years ago

Read 2 more answers

Part 1 of 1 - Question 3 of 20 5.0 Points 2H2 O2 - > 2H2O can be classified as what type of reaction?

mart [117]

2 H₂ + O₂ = 2 H₂O

Answer B only synthesis.

hope this helps!

7 0

3 years ago

A 0.0200 gram piece of unknown alkaline earth metal, M, is reacted with excess 0.500 M H 2 SO 4 , and the hydrogen gas produced

Rama09 [41]

Answer:

0.981atm

Explanation:

According ot Dalton's law total pressure of a mixture of non-reactive gas is equal to sum of partial pressures of individual gases.

total pressure= 1.01at

Number of gases=2

Gases: water vapor and hydrogen

partial pressure of water vapor= 0.029atm

1.01= partial pressure of water vapor+ partial pressure of hydrogen

1.01= 0.029 + partial pressure of hydrogen

partial pressure of hydrogen = 0.981atm

6 0

3 years ago