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3 years ago

B. It shifts the equilibrium toward the right, favoring product.

Chemistry

1 answer:

PilotLPTM [1.2K]3 years ago

8 0

Answer:

11) the difference in heat energies between products and reactants

12) enthalpy change

Explanation:

The heat of reaction is defined as that energy released or absorbed as chemical substances participate in a chemical reaction. It is a term used to denote the change in energy as reactants change into products.

Another name of heat of reaction is enthalpy of reaction. It is a state function since it depends on the initial and final states of the system.

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Which of the following is the test for oxygen has?

dem82 [27]

A or B depends on what you mean by lit or glowing but when you place a wooden split in the sample the gas must reignite but there can be some confusion between hydrogen and oxygen mainly because a splint can cause a slight popping sound while it reignites but hydrogen pops are more violent and can most time extinguish the splint.

5 0

3 years ago

At 1023 K and 1 atm, a 3.00 gram sample of Snoz(s) (gram-formula mass = 151 g/mol) reacts with hydrogen gas to produce tin and w

Blizzard [7]

Answer:

2 moles of Sn are produced when 4 moles of H2(g) are consumed completely

Explanation:

to determine the number of moles of sn (l) produced when 4.0 moles of H2 (g) is consumed completely.

First, find the number of moles of H2 consumed by taking this as limiting reagent.

$n = \frac{g}{M.W (g/mol)}$

Then find the moles of Sn (l) taking into account the stoichiometric relationship between H2(g) and Sn(l). 2:1

$SnO_{2}$ (s) + 2 $H_{2}$ (g) ⇒ Sn(l) + 2 $H_{2}O$ (g)

$mol Sn(l) = \frac{1mol Sn}{2mol H_{2} } . 4 mol H_{2} = 2 mol$

∴2 moles of Sn are produced when 4 moles of H2(g) are consumed completely.

4 0

3 years ago

Suppose there is 0.63 g of HNO3 per 100 mL of a particular solution. What is the concentration of the HNO3 solution in moles per

Vadim26 [7]

Answer:

There are 0.09996826 moles per liter of the solution.

Explanation:

Molar mass of HNO3: 63.02

Convert grams to moles

0.63 grams/ 63.02= 0.009996826

Convert mL to L and place under moles (mol/L)

100mL=0.1 L

0.009996826/0.1= 0.09996826 mol/L

4 0

3 years ago

How many grams of sodium acetate ( molar mass = 83.06 g/mol ) must be added to 1.00 Liter of a 0.200 M acetic acid solution to m

Pie

<u>Answer:</u> The mass of sodium acetate that must be added is 30.23 grams

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

Molarity of acetic acid solution = 0.200 M

Volume of solution = 1 L

Putting values in above equation, we get:

$0.200M=\frac{\text{Moles of acetic acid}}{1L}\\\\\text{Moles of acetic acid}=(0.200mol/L\times 1L)=0.200mol$

To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:

$pH=pK_a+\log(\frac{[\text{salt}]}{[\text{acid}]})$

$pH=pK_a+\log(\frac{[CH_3COONa]}{[CH_3COOH]})$

We are given:

$pK_a$ = negative logarithm of acid dissociation constant of acetic acid = 4.74

$[CH_3COONa]=?mol$

$[CH_3COOH]=0.200mol$

pH = 5.00

Putting values in above equation, we get:

$5=4.74+\log(\frac{[CH_3COONa]}{0.200})$

$[CH_3COONa]=0.364mol$

To calculate the mass of sodium acetate for given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of sodium acetate = 83.06 g/mol

Moles of sodium acetate = 0.364 moles

Putting values in above equation, we get:

$0.364mol=\frac{\text{Mass of sodium acetate}}{83.06g/mol}\\\\\text{Mass of sodium acetate}=(0.364mol\times 83.06g/mol)=30.23g$

Hence, the mass of sodium acetate that must be added is 30.23 grams

7 0

3 years ago

Chem Muti Choice. Tell me the correct answer.

Alex787 [66]

Answer:

my gues is red not a 100% but its in the 700s

Explanation:

3 0

3 years ago

Read 2 more answers