All categories

2 years ago

the actual yield of a certain reaction is 38.0 g while the theoretical yield is 50.0 g calculate the percent yield

Chemistry

1 answer:

Verizon [17]2 years ago

8 0

Answer:

76%

Explanation:

Actual yield = 38.0 g

Theoretical yield = 50.0 g

Percentage yield = ?

The relationship between these quantities is given as;

Percent yield = Actual yield / Theoretical yield * 100%

Percent yield = 38 g / 50 g * 100 %

Percent yield = 0.76 * 100 % = 76%

You might be interested in

Help pls pls pls I really need this answer

blagie [28]

Answer:

I never did this but i think its d 37.5٪ lmk if i got it right pls and srry if i didnt

5 0

3 years ago

What's the importance of anatomy for pharmacy students

Veronika [31]

All health professionals, including pharmacists, must be able to relate form to function..a grounding in anatmony is an essential foundation on which to underpin other knowledge relevant to clinical practice.

3 0

2 years ago

Read 2 more answers

At a constant pressure and amount of gas, how are temperature and volume related?

RSB [31]

The volume is directly proportional to the absolute temperature so the answer is A.

7 0

3 years ago

Determine the mole fraction of the solute if you have 3.4 grams KCl in 8.1 grams H2O

Yakvenalex [24]

.42; 3.4 divided by 8.1 is about .42

6 0

3 years ago

Read 2 more answers

Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Brz(9) 2NOBr(g) A reaction mixture was found to contain 2.69x1

bekas [8.4K]

Explanation:

$2NO(g) + Br_2(g)\rightleftharpoons 2NOBr(g)$

Equilibrium constant of reaction = $K=154$

Concentration of NO = $[NO]=\frac{2.69\times 10^{-2} mol}{1 L}=2.69\times 10^{-2} M$

Concentration of bromine gas = $[Br_2]=\frac{3.85\times 10^{-2} mol}{1 L}=3.85\times 10^{-2} M$

Concentration of NOBr gas = $[Br_2]=\frac{9.56\times 10^{-2} mol}{1 L}=9.56\times 10^{-2} M$

The reaction quotient is given as:

$Q=\frac{[NOBr]^2}{[NO]^2[Br_2]}=\frac{(9.56\times 10^{-2} M)^2}{(2.69\times 10^{-2} M)^2\times 3.85\times 10^{-2} M}$

$Q=328.06$

$Q>K$

The reaction will go in backward direction in order to achieve an equilibrium state.

1. In order to reach equilibrium NOBr (g) must be produced. False

2. In order to reach equilibrium K must decrease. False

3. In order to reach equilibrium NO must be produced. True

4. Q. is less than K . False

5. The reaction is at equilibrium. No further reaction will occur. False

8 0

2 years ago