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DENIUS [597]
2 years ago
11

In an experiment, calcium carbonate reacted with different volumes of hydrochloric acid in water. One of the products formed dur

ing the experiment was carbon dioxide. The time taken for 0.89 mL of carbon dioxide to form was recorded. A partial record of the experiment is shown. Experimental Record Flask Mass of Calcium Carbonate Volume of HCl Volume of Water Time 1 4.0 g 25 mL 0 mL 11.2 seconds 2 4.0 g 20 mL 5 mL 3 4.0 g 15 mL 10 mL 4 4.0 g 10 mL 15 mL

Chemistry
1 answer:
Arte-miy333 [17]2 years ago
5 0

Answer:

12.8seconds, 14.6seconds, 16.4seconds

Explanation:

the answers should b right as long as it is increasing in trend.

the reason why is bc of lower vol of hcl, and higher vol of water present. there is amount of hcl molecules present per volume. lesser chance of collisions, lower rate of successful collisions to poduce CO2

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How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? cacl2(aq) + k2co3(aq) → 2 kcl(aq) + caco3
Virty [35]
CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq)

1.12 g
2.23 g
0.896 g
4.47 g
1.12 g

Hope it helps :)
8 0
2 years ago
Read 2 more answers
For the reaction A+B↽−−⇀C+D, assume that the standard change in free energy has a positive value. Changing the conditions of the
77julia77 [94]

Explanation:

a. Adding a catalyst

no effect .( Catalyst can only change the activation energy but not the free energy).

b. increasing [C] and [D]

Increase the free energy .

c. Coupling with ATP hydrolysis

decrease the free energy value .

d.Increasing [A] and [B]

decrease the free energy.

7 0
2 years ago
What happened to the volume of gas when the syringe was exposed to various temperature conditions? Using the concepts explored i
rewona [7]

Answer:

Thus, when the volume of the gas is exposed to a temperature above -273.15 K, the volume increases linearly with the temperature.

Explanation:

The expression for Charles's Law is shown below:

\frac {V_1}{T_1}=\frac {V_2}{T_2}

This states that the volume of the gas is directly proportional to the absolute temperature keeping the pressure conditions and the moles of the gas constant.

<u>Thus, when the volume of the gas is exposed to a temperature above -273.15 K, the volume increases linearly with the temperature. </u>

<u>For example , if the temperature of the gas is reduced to half, the volume also reduced to half. </u>

<u>At -273.15 K, according to Charles's law, it is possible to make the volume of an ideal gas = 0.</u>

5 0
2 years ago
A 2135 cm3 sample of dry air has a pressure of 98.4 kpa at 127 degrees Celsius. What is the volume of the sample if the Temperat
kykrilka [37]

the equation is p1 x v1 divided by T1 = p1 x v2 = T2 but since the pressure is kept constant you do not even need it so the equation would now be v1 divided by t1 = v2 divided by t2

2135 cm3 divided by 127 degrees celcius = x divided by 206

answer: 3460 cm3

7 0
2 years ago
Read 2 more answers
A chemical engineer calculated that 15.0 mol H2 was needed to react with excess N2 to prepare 10.0 mol NH3. But the actual yield
rjkz [21]

Answer:

The actual number of moles is 9 moles.

It is less than 15

Number of moles needed is 9 moles

Explanation:

15H2 + 10N2 ——-> 10NH3

Now from the question, we can see that the percentage yield is 60%

The percentage yield can be calculated as actual moles of H2/Theoretical moles of H2 * 100%

From the equation, we can see that the theoretical number of moles of hydrogen is 15.

Now to get the actual : 60 = x/15 * 100

x = 9

The actual number of moles is 9 moles.

It is less than 15

Number of moles needed is 9 moles

8 0
2 years ago
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