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3 years ago

Consider this reaction: KOH + HBr --> KBr + H2O

Chemistry

2 answers:

True [87]3 years ago

7 0

Answer:

B) It turns clear phenolphthalein pink.

Explanation:

KOH is a basic solution.

It turns red litmus paper turns blue.

It turns clear phenolphthalein pink.

The reagent which reacts with metals to form hydrogen gas is acid.

So, the right choice is:

B) It turns clear phenolphthalein pink.

Ymorist [56]3 years ago

5 0

Answer : the answer is B

Explanation: it turns clear phenolphthein pink

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Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric che

Helga [31]

Answer:

Partial pressure of dinitrogen tetroxide after equilibrium is reached the second time is 0.82 atm.

Explanation:

$2NO_2(g)\rightleftharpoons N_2O_4(g)$

Initially

3.0 atm 0

At equilibrium

(3.0-2p) p

Equilibrium partial pressure of $NO_2=2.1atm=3.0-2p$

p = 0.45 atm

The value of equilibrium constant wil be given by :

$K_p=\frac{p_{N_2O_4}}{(p_{NO_2})^2}=\frac{p}{(3.0-2p)^2}$

$K_p=\frac{0.45}{(2.1)^2}=0.10$

After addition of 1.5 atm of nitrogen dioxide gas equilibrium reestablishes it self :

$2NO_2(g)\rightleftharpoons N_2O_4(g)$

After adding 1.5 atm of $NO_2$ :

(2.1+1.5) atm 0.45 atm

At second equilibrium:'

(3.6-2P) (0.45+P)

The expression of equilibrium can be written as:

$K_p=\frac{p'_{N_2O_4}}{(p'_{NO_2})^2}$

$0.10=\frac{(0.45+P)}{(3.6-2P)^2}$

Solving for P:

P = 0.37 atm

Partial pressure of dinitrogen tetroxide after equilibrium is reached the second time:

= (0.45+P) atm = (0.45 + 0.37 )atm = 0.82 atm

Partial pressure of dinitrogen tetroxide after equilibrium is reached the second time is 0.82 atm.

5 0

3 years ago

Which property of matter depends on the amount of matter present?

andrew-mc [135]

C.) Volume
Intensive properties, for example; color and density, do not depend on present matter.

8 0

4 years ago

Read 2 more answers

For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction

LUCKY_DIMON [66]

Answer:

The answer to your question is

Explanation:

Data

12.5 g of reactant

Balanced Reaction 1

TiBr₄ + 2H₂ ⇒ Ti + 4HBr

Molar mass of TiBr₄ = 48 + (4 x 80) = 368 g

Atomic mass of Ti = 48 g

Molar mass of HBr = 1 + 80 = 81

368 g of TiBr₄ ---------------- 48 g of Ti

12.5 g of TiBr₄ -------------- x

x = (12.5 x 48) / 368

x = 1.63 g of Ti

368 g of TiBr₄ ----------------4(81) g of HBr

12.5 g of TiBr₄ ------------- x

x = (12.5 x 324) / 368

x = 11 g of HBr

Balanced reaction 2

3SiH₄ + 4NH₃ ⇒ Si₃N₄ + 12H₂

Molar mass of SiH₄ = 28 + 4 = 32

Molar mass of Si₃N₄ = 28 x 3 + 14 x 4 = 84 + 56 = 140 g

Atomic mass of H₂ = 2 g

3(32) g of SiH₄ --------------- 140 g of Si₃N₄

12.5 g of SiH₄ -------------- x

x = 18.2 g of Si₃N₄

3(32) g of SiH₄ --------------- 24 g of H₂

12.5 g of SiH₄ -------------- x

x = 3.125 g of H₂

5 0

4 years ago

Question 6 (1 point)

Mumz [18]

Answer: The answer is MEDUIM

Explanation:

3 0

3 years ago

For the reaction NH4NO3 (s) → N2O (g) + 2H2O (l), you decompose 1 mole NH4NO3 and only get 0.75 moles of N2O. The percent yield

attashe74 [19]

Answer:

The answer to your question is False.

Explanation:

Data

1 mole of NH₄NO₃

0.75 moles of N₂O

Percent yield = 25%

Chemical reaction

NH₄NO₃ ⇒ N₂O + 2H₂O

Process

1.- Determine the theoretical yield

1 mol NH₄NO₃ ------------- 1 mol of N₂O

2.- Calculate the percent yield

Percent yield = Actual yield / Theoretical yield x 100

-Substitution

Percent yield = 0.75 / 1 x 100

-Simplification

Percent yield = 0.75 x 100

-Result

Percent yield = 75%

Conclusion

False, the actual percent yield is 75%

5 0

4 years ago