A gram of gasoline produces 45.0 kJ of energy when burned. Gasoline has a density of 0.77 g/ml. How would you ca the amount of e

B is identified as an ionic compound. Explanation: This conclusion is drawn based on the characteristics of ionic compounds, which typically form crystals similar to salt (sodium chloride), are soluble in water, exhibit high boiling and melting points, possess hardness from strong intermolecular forces, and can conduct electricity—though only when dissolved or in a molten state.

The answer is - 0.138 M. The buffer pH can be determined using the Henderson equation. Here, acts as a weak acid and serves as its corresponding conjugate base. The weak acid has two protons, while the base contains one. The equation can therefore be expressed in terms of protons transferred. Phosphoric acid can donate protons in three stages; the equation we’ve referenced pertains to the second stage, as the acid then has only two protons available and the base only one. Given the concentration of the acid as 0.10 M, we need to calculate the concentration of the base necessary to form a buffer with a pH of exactly 7.0. Substituting the values into the equation leads us to the solution. Cross-multiplying, we find that [base] = 1.38(0.10), yielding [base] = 0.138. Therefore, the concentration of the base needed for the buffer is 0.138 M.

Answer:

9.69g

Explanation:

To find the needed outcome, we first need to determine the number of moles of N2 present in 7.744L of the gas.

1 mole of gas takes up 22.4L at STP.

Thus, X moles of nitrogen gas (N2) will fill 7.744L, meaning

X moles of N2 = 7.744/22.4 = 0.346 moles

Next, we will convert 0.346 moles of N2 to grams to achieve the result sought. The calculation goes as follows:

Molar Mass of N2 = 2x14 = 28g/mol

Number of moles N2 = 0.346 moles

Find the mass of N2 =?

Mass = number of moles × molar mass

Mass of N2 = 0.346 × 28

Mass of N2 = 9.69g

Hence, 7.744L of N2 consists of 9.69g of N2

Answer:- 64015 J

Solution: The calorimeter contains 4250 mL of water, which is at a temperature of 22.55 degrees Celsius.

The water's density is 1 gram per mL.

Thus, the mass of water = = 4250 grams.

After introducing the hot copper bar, the final temperature of the water reaches 26.15 degrees Celsius.

Thus, for the water = 26.15 - 22.55 = 3.60 degrees Celsius.

The specific heat capacity of water is 4.184 .

To determine the heat absorbed by the water, we can use the following formula:

where q represents heat energy, m refers to mass, and c indicates specific heat.

Now let's substitute the values into the equation to perform the calculations:

q = 64015 J

Therefore, the water absorbs 64015 J of heat.

One electron is involved. Explanation: In redox reactions, determining the equivalents requires knowledge of the number of transferred electrons. In this specific case, one equivalent corresponds to a transfer of a single electron.