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2 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]2 years ago

8 0

Answer:

Explanation:

valentinak56 [21]2 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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Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) This reaction is carried out at a different temperature with initial conc

Anni [7]

Answer:

Ka = 4.76108

Explanation:

CO(g) + 2H2(g) ↔ CH3OH(g)

∴ Keq = [CH3OH(g)] / [H2(g)]²[CO(g)]

[ ]initial change [ ]eq

CO(g) 0.27 M 0.27 - x 0.27 - x

H2(g) 0.49 M 0.49 - x 0.49 - x

CH3OH(g) 0 0 + x x = 0.11 M

replacing in Ka:

⇒ Ka = ( x ) / (0.49 - x)²(0.27 - x)

⇒ Ka = (0.11) / (0.49 - 0.11)² (0.27 - 0.11)

⇒ Ka = (0.11) / (0.38)²(0.16)

⇒ Ka = 4.76108

7 0

2 years ago

If 0.35 moles of kcl was dissolved in enough water to make 0.2 L of solution, what is molarity?

Mars2501 [29]

Answer:

1.75M

Explanation:

molarity = number of moles of solute/ number of L of solution =

=0.35 mol/0.2L = 1.75 mol/L = 1.75 M

8 0

2 years ago

Is a oreo a pure substance or a mixture

adoni [48]

Belive it or not but an oreo is a mixture. LOL

7 0

2 years ago

How many Joules are released to cool 250.0 grams of liquid water from 100°C to 0°C? The specific heat of water is 4.180 J/g.C.

nlexa [21]

$\bold{\huge{\orange{\underline{ Solution}}}}$

$\bold{\underline{ Given :- }}$

We have 250g of liquid water and it needs to be cool at temperature from 100° C to 0° C
Specific heat of water is 4.180J/g°C

$\bold{\underline{ To \: Find :- }}$

We have to find the total number of joules released.

$\bold{\underline{ Let's \:Begin:- }}$

We know that,

Amount of heat energy = mass * specific heat * change in temperature

That is, 

$\sf{\red{ Q = mcΔT }}$

Subsitute the required values in the above formula :-

$\sf{ Q = 250 × 4.180 ×(0 - 100 )}$

$\sf{ Q = 250 × 4.180 × - 100 }$

$\sf{ Q = 250 × - 418}$

$\sf{\pink{ Q = - 104,500 J }}$

Hence, 104,500 J of heat is released to cool 250 grams of liquid water from 100° C to 0° C.

$\bold{\underline{ Now :- }}$

We have to tell whether the above process is endothermic or exothermic :-

Here, In the above process ΔT is negative and as a result of it Q is also negative that means above process is Exothermic

Exothermic process :- It is the process in which heat is evolved .
Endothermic process :- It is the process in which heat is absorbed .

4 0

1 year ago

The air all around us is a mixture of gasses containing nitrogen, oxygen, carbon dioxide, argon

KiRa [710]

Answer:

Total pressure = 4.57 atm

Explanation:

Given data:

Partial pressure of nitrogen = 1.3 atm

Partial pressure of oxygen = 1824 mmHg

Partial pressure of carbon dioxide = 247 torr

Partial pressure of argon = 0.015 atm

Partial pressure of water vapor = 53.69 kpa

Total pressure = ?

Solution:

First of all we convert the units other into atm.

Partial pressure of oxygen = 1824 mmHg / 760 = 2.4 atm

Partial pressure of carbon dioxide = 247 torr / 760 = 0.325 atm

Partial pressure of water vapor = 53.69 kpa / 101 = 0.53 atm

Total pressure = Partial pressure of N + Partial pressure of O + Partial pressure of CO₂ + Partial pressure of Ar + Partial pressure of water vapor

Total pressure = 1.3 atm + 2.4 atm + 0.325 atm + 0.015 atm + 0.53 atm

Total pressure = 4.57 atm

4 0

3 years ago