All categories

3 years ago

Which reactants would lead to a spontaneous reaction?

1 answer:

5 0

The reactants that would lead to a spontaneous reaction are Mn2+ and Al3+. Al and Mn are not because they are stable reactants. Mn and Al3+ are not because Mn is stable. Mn2+ and Al are not because Al is stable.

You might be interested in

What is the density of an object with a mass of 16 g and 3.0 ml

fomenos

Answer:

D = 5.3 g/mL

Explanation:

Density = Mass over Volume

D = m/V

Step 1: Define

D = unknown

m = 16 g

v = 3.0 mL

Step 2: Substitute and Evaluate

D = 16 g / 3.0 mL

D = 5.333333333 g/mL

Step 3: Simplify

We have 2 sig figs.

5.333333333 g/mL ≈ 5.3 g/mL

6 0

3 years ago

Which one of the following items does NOT characterize a reducing agent? a. A reducing agent loses electrons. b. A reducing agen

Ad libitum [116K]

Answer: D

Explanation:

A reducing agent is a species that reduces other compounds, and is thereby oxidized. The whole compound becomes the reducing agent. In other words, of a compound is oxidized, then they are the reducing agent. On the other hand, if the compound is reduced, it is an ozidizing agent.

Since we have established that a reducing agent is the compound being oxidized, we know that A is not our answer. An oxidized compound is losing electrons. Choice A states exactly this.

For B, this is true as we have established this already.

C is also correct. Since a reducing agent loses electrons, it becomes more positive. This makes the oxidation number increase.

D would be our correct answer. It is actually a good oxidizing agent is a metal in a high oxidation state, such as Mn⁷⁺.

4 0

2 years ago

_____ were common ocean scavengers long ago, and they are frequently found in fossilized form.

quester [9]

Answer:

a. trilobites.

Explanation:

6 0

3 years ago

A solution is prepared by mixing 93.0 mL of 5.00 M HCl and 37.0 mL of 8.00 M HNO3. Water is then added until the final volume is

Charra [1.4K]

Answer:

$[H^{+}] = 0.761 \frac{mol}{L}$

$[OH^{-}]=1.33X10^{-14}\frac{mol}{L}$

$pH = 0.119$

Explanation:

HCl and HNO₃ both dissociate completely in water. A simple method is to determine the number of moles of proton from both these acids and dividing it by the total volume of solution.

$n_{H^{+} } from HCl = [HCl](\frac{mol}{L}). V_{HCl}(L) \\ n_{H^{+} } from HNO_{3} = [HNO_{3}](\frac{mol}{L}). V_{HNO_{3}}(L)$

Here, n is the number of moles and V is the volume. From the given data moles can be calculated as follows

$n_{H^{+} } from HCl = (5.00)(0.093)$

$n_{H^{+} } from HCl = 0.465 mol$

$n_{H^{+} } from HNO_{3} = (8.00)(0.037)$

$n_{H^{+} } from HNO_{3} = 0.296 mol$

$n_{H^{+}(total) } = 0.296 + 0.465$

$n_{H^{+}(total) } = 0.761 mol$

For molar concentration of hydrogen ions:

$[H^{+}] = \frac{n_{H^{+}}(mol)}{V(L)}$

$[H^{+}] = \frac{0.761}{1.00}$

$[H^{+}] = 0.761 \frac{mol}{L}$

From dissociation of water (Kw = 1.01 X 10⁻¹⁴ at 25°C) [OH⁻] can be determined as follows

$K_{w} = [H^{+} ][OH^{-} ]$

$[OH^{-}]=\frac{Kw}{[H^{+}] }$

$[OH^{-}]=\frac{1.01X10-^{-14}}{0.761 }$

$[OH^{-}]=1.33X10^{-14}\frac{mol}{L}$

The pH of the solution can be measured by the following formula:

$pH = -log[H^{+} ]$

$pH = -log(0.761)$

$pH = 0.119$

5 0

2 years ago

Would precipitation occur when 500 mL of a 0.02M solution of $AgNO_3$ is mixed with 500 mL of a 0.001M solution of NaCl? Show

stira [4]

The balanced chemical reaction is
NaCl + AgNO3 --> AgCl + NaNO3
To find out if precipitation will occur, we need to calculate the number of
moles acting in the chemical reaction
But Molarity, M=nV, where n is the number of moles and V is the volume in
litres. So n = M/V
number of moles of AgNo3 = 0.02/500 * 10^(-3)
n= 0.04
While n of Sodium chloride = 0.01/0.5 = 0.2. Since there is excess sodium chloride ( twice as much) precipitation will not occur. 2NaCl + 2AgNO3 -->
2AgCl + 2NaNO3. The reaction requires one and not two moles of AgNo3 as evident from the number of moles which is 0.04

4 0

2 years ago