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3 years ago

If 2.00 g of Zn is allowed to react with 2.00 g of CuSO4, how many grams of

Chemistry

2 answers:

otez555 [7]3 years ago

8 0

Answer:

Explanation:

valentinak56 [21]3 years ago

7 0

Answer:

1.1445g

Explanation:

Mass of Zn = 2.0g

Mass of CuSO4 = 2.0g

Molar mass of Zn = 65.4g/mol

Molar mass of CuSO4 = 159.5g/mol

No. Of moles = mass / molar mass

No. Of moles of Zn = 2.0/65.4 = 0.030moles

No. Of moles of CuSO4 = 2/159.5 = 0.0125 moles

Equation of reaction

CuSO4 (aq) +Zn(s)-> ZnSO4(aq) + Cu(s)

Stoichiometric molar ratio of CuSo4 : Zn = 1:1

Actual molar ration of CuSO4 : Zn = ?

0.0125 / 0.030 = 1 / 2.4

Zn is present in excess in the reaction, while CuSO4 is the limiting reagent

1 mol of CuSO4 = 1 mol of Zn

0.0125 moles of CuSO4 = 0.0125 moles of Zn

No. Of moles left after reaction = 0.030 - 0.0125 = 0.0175 moles.

Mass = no. Of moles * molar mass = 0.0175 * 65.4 = 1.1445g

The mass of Zn left after the reaction is 1.1445g.

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an ideal gas is at a pressure 1.00 x 10^5 N/m^2 and occupies a volume 11.00 m^3. If the gass is compressed to a volume of 1.00 m

bogdanovich [222]

Answer:

$P_2=1.1x10^6Pa$

Explanation:

Hello.

In this case, we can solve this problem by applying the Boyle's law which allows us to understand the pressure-volume behavior as a directly proportional relationship:

$P_1V_1=P_2V_2$

In such away, knowing the both the initial pressure and volume and the final volume, we can compute the final pressure as shown below:

$P_2=\frac{P_1V_1}{V_2}$

Consider that the given initial pressure is also equal to Pa:

$P_2=\frac{1.00x10^5Pa*11.00m^3}{1.00m^3}\\ \\P_2=1.1x10^6Pa$

Which stands for a pressure increase when volume decreases.

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4 0

3 years ago

Which best describes a neutralization reaction?

Softa [21]

A reaction between to acids

3 0

4 years ago

What happens to the atoms during a chemical reaction

Likurg_2 [28]

Answer:

Atoms get rearranged and make up different molecules. No atoms are created nor destroyed.

Explanation:

6 0

2 years ago

When 4.15 grams of silver nitrate is reacted with 1.11 grams of iron(III) chloride, which best represents the amount of silver c

PolarNik [594]

Answer:

The mass of silver chloride produced = 2.202 g

Explanation:

Equation of the reaction is given below

3AgNO₃(aq) + FeCl₃(aq) ----> 3AgCl(s) + Fe(NO₃)₃(aq)

molar mass of AgNO₃ = 170 g/mol

molar mass of FeCl₃ = 233.5 g/mol

molar mass of AgCl = 143.5 g/mol

3 moles of silver nitrate reacts with 1 mole of iron (iii) chloride to give 3 moles of silver nitrate

4.15 grams of AgNO₃ = 4.15/170 = 0.0244 moles of AgNO₃

1.11 grams of FeCl₃ = 1.11/233.5 = 0.0047 moles of FeCl₃

mole ratio of AgNO₃ to FeCl₃ = 0.0244/0.0047 = 5 : 1

therefore, FeCl₃ is the limiting reactant

0.0047 moles of FeCl₃ reacting will produce 0.0047 * 3 moles of AgCl = 0.0141 moles of AgCl

0.0141 moles of AgCl = 0.0141 * 143.5 g of AgCl = 2.02 g of AgCl =

Therefore mass of silver chloride produced = 2.202 g

3 0

3 years ago

Find the celcius equivalent of 133 degrees Kelvin

egoroff_w [7]

Answer:

Explanation:

To convert a temperature from degree Celsius to Kelvin add 273 to the value in degree Celsius

That's

K = 273 + °C

where

K is the temperature in Kelvin

°C is the temperature in degree Celsius

From the question we have

K = 273 + 133

We have the final answer as

Hope this helps you

5 0

3 years ago

Read 2 more answers