In a reaction Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq), 6.00 g of Mg was present at 0.00 min. After 3.00 min, 4.50 g of Mg remained. Express the average rate as mol of Mg consumed per minute.

I was taught how to use molarity but this question does not tell me molarity, just grams so I do not know how to solve it.

Mrbob222 can you make it clear a little bit cuz 👴🏻👓🤏🏻 GOD DAHYUM. I did not get that😩

Just convert grams Mg to mols Mg and you have it.

g Mg/min = 1.5/3.0 = 0.5 g Mg/min or 0.5 g/24.3 = approx 0.02 mol Mg/min.

or convert at the beginning but it's more work.
6.00/24.3 = approx 0.25 mols Mg initially.
4.50/24.3 = approx 0.19 mols final.
(delta mols Mg) = approx 0.25-0.19 = about 0.06 mol Mg/3.00 min or about 0.02 mol Mg/min.

Lmao so guys what the answer i need it for my homework 💀

Well, it seems like you're in a bit of a pickle! But fear not, my friend, Clown Bot is here to lend a hand, or rather a joke!

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Now, back to your question. Don't worry about the molarity, we can solve this using good old-fashioned stoichiometry! Let's break it down step by step:

Step 1: Calculate the number of moles of Mg initially present.
You have 6.00 g of Mg and the molar mass of Mg is approximately 24.31 g/mol. So, using the formula mass/ molar mass, we get:
moles of Mg = 6.00 g / 24.31 g/mol = 0.2468 mol

Step 2: Calculate the number of moles of Mg consumed.
After 3.00 minutes, you have 4.50 g of Mg remaining. Using the same formula as before, we get:
moles of Mg consumed = (6.00 g - 4.50 g) / 24.31 g/mol = 0.0617 mol

Step 3: Calculate the average rate of Mg consumption.
To find the average rate, we divide the moles of Mg consumed by the time in minutes:
average rate = (0.0617 mol) / (3.00 min) ≈ 0.0206 mol/min

Tada! The average rate of Mg consumption is approximately 0.0206 mol/min. So there you have it, a solution disguised as a joke! Keep up the great work, my friend!

To determine the average rate of the reaction in terms of moles of magnesium (Mg) consumed per minute, we need to use the given masses of Mg.

First, convert the mass of Mg to moles using the molar mass of Mg. The molar mass of Mg is 24.31 g/mol.

The initial number of moles of Mg (n(initial)) can be calculated as follows:
n(initial) = mass(initial) / molar mass(Mg)
n(initial) = 6.00 g / 24.31 g/mol

Next, calculate the final number of moles of Mg (n(final)) using the remaining mass of Mg after 3.00 minutes:
n(final) = mass(final) / molar mass(Mg)
n(final) = 4.50 g / 24.31 g/mol

Now, calculate the change in moles (Δn) of Mg during the reaction:
Δn = n(final) - n(initial)

Finally, calculate the average rate of the reaction as moles of Mg consumed per minute:
average rate = Δn / Δt
Here, Δt is the change in time. From the given information, Δt = 3.00 minutes.

average rate = Δn / Δt
average rate = (n(final) - n(initial)) / Δt

Now, substitute the calculated values to find the average rate of the reaction in moles of Mg consumed per minute.