A sample of aluminum requires 341 J of energy to raise the temperature from 18.0ºC to 55.0ºC. Calculate the mass of the aluminum sample.

10.22g

Explanation:

Using the formula as follows:

Q = m × c × ∆T

Where;

Q = amount of heat required (J)

m = mass of substance (g)

c = specific heat of substance (J/g°C)

∆T = change in temperature (°C)

According to the information given in this question;

Q = 341J

m = ?

∆T = 55.0ºC - 18.0ºC = 37°C

c of aluminum = 0.902J/g°C

Using Q = m × c × ∆T

341 = m × 0.902 × 37

341 = 33.374m

m = 341 ÷ 33.374

m = 10.22g

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

- calcium has greater affinity to bond with electron receptors than hydrogen does and hence, it has the ability to replace hydrogen in most of its compounds.

- lithium has 2 valence electrons in the product because it can make only 1 bond with hydrogen. beryllium has 4 valence electrons in the product because it can only make 2 bonds. it has fewer electrons than neon and can react with electron donors. each hydrogen has 2 valence electrons, the same as helium.

- the covalent bond formed between carbon and hydrogen is polar because carbon is more electronegative than hydrogen and it attracts the bonded electron pair closer to itself, thus giving hydrogen a partial positive charge.

- a hydrogen bond is a relatively weak bond that hydrogen atoms make with the electronegative atoms nitrogen, oxygen or fluorine.

so the best choice is a.) 2 calcium (ca) atoms