PLS HELP ASAP WITH SCIENCE HW

The Haber Process is the main industrial procedure to produce ammonia. The reaction combines nitrogen from air with hydrogen mai

Firdavs [7]

Answer:

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

B) $Kc=0.0933$ .

C) 0.9 mol.

D) Increasing both temperature and pressure.

Explanation:

Hello,

In this case, given the information, we proceed as follows:

A)

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

B) For the calculation of Kc, we rate the equilibrium expression:

$Kc=\frac{[NH_3]^2}{[N_2][H_2]^3}$

Next, since at equilibrium the concentration of ammonia is 0.6 M (0.9 mol in 1.5 dm³ or L), in terms of the reaction extent $x$ , we have:

$[NH_3]=0.6M=2*x$

$x=\frac{0.6M}{2}=0.3M$

Next, the concentrations of nitrogen and hydrogen at equilibrium are:

$[N_2]=\frac{1.5mol}{1.5L}-x=1M-0.3M=0.7M$

$[H_2]=\frac{4mol}{1.5L}-3*x=2.67M-0.9M=1.77M$

Therefore, the equilibrium constant is:

$Kc=\frac{(0.6M)^2}{(0.7M)*(1.77M)^3}\\ \\Kc=0.0933$

C) In this case, the equilibrium yield of ammonia is clearly 0.9 mol since is the yielded amount once equilibrium is established.

D) Here, since the reaction is endothermic (positive enthalpy change), one way to increase the yield of ammonia is increasing the temperature since heat is reactant for endothermic reactions. Moreover, since this reaction has less moles at the products, another way to increase the yield is increasing the pressure since when pressure is increased the side with fewer moles is favored.

Best regards.

7 0

2 years ago

The diagram below shows a gas sample being measured with an open-end mercury (Hg) manometer. If a barometer reads 730. 1 torr, w

IRISSAK [1]

The pressure of the gas in the flask (in atm) when Δh = 5.89 cm is 1.04 atm

<h3>Data obtained from the question</h3>

The following data were obtained from the question:

Atmospheric pressure (Pa) = 730.1 torr = 730.1 mmHg
Change in height (Δh) = 5.89 cm
Pressure due to Δh (PΔh) = 5.89 cmHg = 5.89 × 10 = 58.9 mmHg
Pressure of gas (P) =?

<h3>How to determine the pressure of the gas</h3>

The pressure of the gas can be obtained as illustrated below:

P = Pa + PΔh

P = 730.1 + 58.9

P = 789 mmHg

Divide by 760 to express in atm

P = 789 / 760

P = 1.04 atm

Thus, the pressure of the gas when Δh = 5.89 cm is 1.04 atm

Learn more about pressure:

brainly.com/question/22523697

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Missing part of question:

See attached photo

5 0

1 year ago

1. A 25 g rock is placed in a graduated cylinder with water. The volume of the liquid rises from 18.3 mL to 21.4 mL Calculate th

MaRussiya [10]

Answer:

1. $\rho=8.06g/cm^3$

2. $H=10cm$

Explanation:

Hello,

1. In this case, since the volume of the rock is obtained via the difference between the volume of the cylinder with the water and the rock and the volume of the cylinder with the water only:

$V=21.4mL-18.3mL=3.1mL$

Thus, the density turns out:

$\rho=\frac{m}{V}=\frac{25g}{3.1cm^3} \\\\\rho=8.06g/cm^3$

2. In this case, given the density and mass of aluminum we can compute its volume as follows:

$V=\frac{m}{\rho}=\frac{1080g}{2.7g/cm^3}=400cm^3$

Moreover, as the volume is also defined in terms of width, height and length:

$V=W*H*L$

The height is computed to be:

$H=\frac{V}{L*W}=\frac{400cm^3}{5cm*8cm}\\ \\H=10cm$

Best regards.

3 0

2 years ago

Part

r-ruslan [8.4K]

The molar concentration will be greater than 0.01 M $KIO_{3}$ .

Since more of the compound was measured out than what was calculated, you can think of the solution as being 'stronger' than what it was calculated to be. Since a 'stronger' concentration results in a number that is higher, the molarity of this solution is going to be greater than 0.01 M.

7 0

2 years ago

What is the empirical formula of C6H12O6?<br><br> C2H4O2<br> CH2O<br> CH2O2<br> C2H4O

wariber [46]

Answer: The empirical formula for C6H12O6 is CH2O. Every carbohydrate, be it simple or complex, has an empirical formula CH2O

Explanation:

5 0

1 year ago