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miskamm [114]
2 years ago
14

Consider the following reaction and situations 1 through 10. In the spaces provided, clearly indicate the best response to each

situation. A. increase C. no change E. shift right B. decrease D. shift left F. cannot be determined C(s) + H2O(g) ⇌ CO(g) + H2(g) H > 0 _____ 1. What will be the effect upon the equilibrium if the pressure on the system is increased? _____ 2. What will be the effect upon the concentration of CO if the concentration of H2 is decreased? _____ 3. What will be the effect upon the equilibrium if the concentration of H2 is decreased? _____ 4. What will be the effect upon the concentration of H2O if the concentration of H2 is increased? _____ 5. What will be the effect upon the equilibrium if H2 is removed and more C is added? _____ 6. What will be the effect upon the concentration of H2 if the amount of C is increased? _____ 7. What will be the effect upon the equilibrium if the temperature and the concentration of H2 increases? _____ 8. What will be the effect upon the concentration of CO if the temperature is increased? _____ 9. What will be the effect upon the equilibrium if the concentration of H2O is decreased and CO is increased? _____ 10. What will be the effect upon the equilibrium if a catalyst is added?
Chemistry
1 answer:
olchik [2.2K]2 years ago
5 0

Answer:

1. C. no change

2. A. increase

3. E. shift to the right

4. A. increase

5. E. shift to the right

6. A. increase

7. F. cannot be determined

8. B increase

9. D. shift to the left

10 F. cannot be determined

Explanation:

<em>According to Le Chaterlier principle, when a reaction is in equilibrium and one of the constraints that affect reactions is applied, the equilibrium will shift so as annul the effects of the constraints.</em>

From the equation: C(s) + H2O(g) ⇌ CO(g) + H2(g),

H is greater than 0, meaning that the system is endothermic, that is energy is absorbed.

1. If the pressure of the system is increased, there would be no change to the system because there are equal number of moles of products and reactants.

2. If H2 concentration is decreased, the equilibrium will shift to the right and more products will be formed. Hence, the concentration of CO will increase.

3. If H2 concentration is decreased, the equilibrium will shift to the right to annul the effects of the decrease in the concentration of a product.

4. If the concentration of H2 is increased, the equilibrium will shift to the left to annul the effects of increased concentration of a product. Hence, more H2O would be formed.

5. If H2 (a product) is removed, and C (a reactant) is added, more of the products will be formed in order to annul the effects of the actions. Hence, equilibrium will shift to the right.

6. If the amount of C (a reactant) is increased, the equilibrium will shift to the right. Hence, more H2 will be formed.

7. The reaction is endothermic, hence an increase in temperature will ordinarily shift the equilibrium to the right. However, the addition of H2 (a product) is supposed to shift the equilibrium to the left. Hence, the effects of simultaneous addition of the two actions become indeterminate.

8. Since the reaction is endothermic, increase in the temperature of the system will shift the equilibrium to the right. Hence, more CO will be formed.

9. If the concentration of H2O (a reactant) is decreased and that of CO (a product) is increased, both actions lead to the equilibrium being shifted to the left.

10. Addition of catalyst to the system will only speed up the rate at which the system reach the equilibrium.

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Number of grams of hcl that can react with 0.500 grams of Al(OH)3
vlabodo [156]

Answer:

0.7g of HCl

Explanation:

First, let us write a balanced equation for the reaction between HCl and Al(OH)3.

This is illustrated below:

Al(OH)3 + 3HCl —> AlCl3 + 3H2O

Next, let us obtain the masses of Al(OH)3 and HCl that reacted together according to the equation. This can be achieved as shown below:

Molar Mass of Al(OH)3 = 27 + 3(16+1)

= 27 + 3(17) = 27 + 51 = 78g/mol.

Molar Mass of HCl = 1 + 35.5 = 36.5g/mol

Mass of HCl from the balanced equation = 3 x 36.5 = 109.5g

Now we can obtain the mass of HCl that would react with 0.5g of Al(OH)3. This can be achieved as follow:

Al(OH)3 + 3HCl —> AlCl3 + 3H2O

From the equation above,

78g of Al(OH)3 reacted with 109.5g of HCl.

Therefore, 0.5g of Al(OH)3 will react with = (0.5 x 109.5)/78 = 0.7g of HCl

7 0
3 years ago
Given the equation I = Q/t, solve for t.
larisa86 [58]

Answer: t=\frac{Q}{I}

Explanation:

I=\frac{Q}{t}

Multiply by t on both sides.

t*I=\frac{Q}{t}*t

tI=Q

Now divide by I to isolate t.

\frac{tI}{I}=\frac{Q}{I}

t=\frac{Q}{I}

5 0
3 years ago
The specific heat of copper is 0.40 joules/ g °c. How much heat is needed in joules to change the temperature of a 55 gram subst
Snezhnost [94]

Answer : The amount of heat needed is, 1188 J

Explanation :

Formula used :

q=m\times c\times (T_2-T_1)

where,

q = heat needed = ?

m = mass of copper = 55 g

c = specific heat capacity of copper = 0.40J/g^oC

T_1 = initial temperature = 20.0^oC

T_2 = final temperature = 74.0^oC

Now put all the given values in the above formula, we get:

q=55g\times 0.40J/g^oC\times (74.0-20.0)^oC

q=1188J

Thus, the amount of heat needed is, 1188 J

3 0
3 years ago
Which element would mostly have chemical properties similar to that of magnesium (Mg)?
DanielleElmas [232]

The elements of same group are placed in same group as they have similar properties. So Calcium is the element which resembles Mangesium.

Calcium and Magnesium both are alkaline earth metals.

They have similar properties as they have similar outer or valence shell electronic configuration

The general electronic configuration of alkaline earht metal is ns2

The electronic configuration of Mg [atomic number 12] and Ca [atomic number 20] are

[Ne]3s^{2}  and [Ar]4s^{2} respectively.


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3 years ago
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Answer:

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