2 years ago

WILL MARK BRAINLIEST IF YOU ANSWER EVERY QUESTION!!!!

Chemistry

1 answer:

Savatey [412]2 years ago

4 0

Answer:

The answer for number one is .A

The answer for number two is heat rises

Explanation:

You might be interested in

Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left

Vera_Pavlovna [14]

So C12 is the limiting reactant and P4 is the excess
Mass P4 consumed= 0.31 mol X 123.9 g/mol =38.41 g P4 consumed.
Hope i helped

6 0

3 years ago

For the oxidation of ammonia

OverLord2011 [107]

The answer is 0.405 M/s

- (1/3) d[O2]/dt = 1/2 d[N2]/dt

- d[O2]/dt = 3/2 d[N2]/dt

- d[O2]/dt = 3/2 × 0.27

- d[O2]/dt = 0.405 mol L^(-1) s^(-1)

5 0

2 years ago

State the Periodic Law. Why is it so important in the study of chemistry?

gayaneshka [121]

Answer:

Summary. To summarize, the periodic table is important because it is organized to provide a great deal of information about elements and how they relate to one another in one easy-to-use reference. The table can be used to predict the properties of elements, even those that have not yet been discovered.

8 0

3 years ago

Calculate the mass of Iron in 40g of Fe203

Nat2105 [25]

Answer:

‏‏‎ ‎

Explanation:‏‏‎ ‎‏‏‎ ‎‏‏‎ ‎

7 0

2 years ago

Which direction will the following reaction (in a 5.0 L flask) proceed if the pressure of CO_2(g) is 1.0 atm? CaCO_3(s) rightarr

storchak [24]

Answer:

d. To the left because Q > K_p

Explanation:

Hello,

In this case, for the given reaction:

$CaCO_3(s) \rightarrow CaO(s) + CO_2(g)$

The pressure-based equilibrium expression is:

$Kp=p_{CO_2}$

In such a way, since Kp is given we rather compute the reaction quotient at the specificed pressure of carbon dioxide as shown below:

$Q=p_{CO2}=1.0$

Therefore, since Q>Kp we can see that there are more products than reactants, which means that the reaction must shift leftwards towards the reactants in order to reestablish equilibrium, thus, answer is d. To the left because Q > Kp.

Regards.

6 0

3 years ago