Consider:
C(12)H(22)O(11)(s)-->(11)H(2O)(g)+(12)C(s)
The rate of decomposition of C12H22O11 is 0.75 mol/min. What mass of C is produced in 10 seconds?
0.75 mols/min x(1 min/60 s) x 10 s = approx 0.12 mols C12H22O11 in 10 s.
You get 12 times that C so you have 0.12 x 12 = approx 1.5 mol C and that x atomic mass C = grams.
Remember those first numbers are approximations so you should recalculate from the beginning.
The answer isn't 18 g/s; it's 18 g/10 seconds and problem asked for grams in 10 seconds.
To find the mass of carbon (C) produced in 10 seconds, we need to follow these steps:
Step 1: Calculate the molar mass of C12H22O11
Step 2: Determine the moles of C produced in 10 seconds
Step 3: Calculate the mass of C produced in 10 seconds
Let's calculate step-by-step.
Step 1: Calculate the molar mass of C12H22O11
The molar mass of C12H22O11 can be calculated by adding up the atomic masses of each element present.
C: 12.01 g/mol
H: 1.01 g/mol
O: 16.00 g/mol
Molar mass of C12H22O11 = (12.01 * 12) + (1.01 * 22) + (16.00 * 11)
= 144.12 + 22.22 + 176.00
= 342.34 g/mol
Step 2: Determine the moles of C produced in 10 seconds
The balanced chemical equation tells us that for every 12 moles of C12H22O11 decomposed, 12 moles of C are produced.
The rate of decomposition of C12H22O11 is given as 0.75 mol/min.
We need to convert the given rate from mol/min to mol/second:
0.75 mol/min * (1 min/60 s) = 0.0125 mol/s
Since the ratio of C12H22O11 to C is 1:1, the moles of C produced in 10 seconds would be:
Moles of C produced = 0.0125 mol/s * 10 s
= 0.125 mol
Step 3: Calculate the mass of C produced in 10 seconds
We can use the molar mass of C (12.01 g/mol) to calculate the mass of C produced.
Mass of C = Moles of C produced * Molar mass of C
= 0.125 mol * 12.01 g/mol
= 1.50125 g
≈ 1.50 g
Therefore, the mass of carbon (C) produced in 10 seconds is approximately 1.50 grams.
To determine the mass of C produced in 10 seconds, we first need to find the molar mass of C, which is approximately 12.01 g/mol.
Given that the rate of decomposition of C12H22O11 is 0.75 mol/min, we can calculate the moles of C produced in 10 seconds by using the ratio of C12H22O11 to C.
The balanced equation shows that for every 12 moles of C12H22O11 decomposed, 12 moles of C are produced. Thus, the mole ratio of C12H22O11 to C is 1:1.
Now, let's calculate the moles of C produced in 10 seconds:
0.75 mol/min * (10 seconds / 60 seconds) = 0.125 mol
Since we know the mole ratio is 1:1, the moles of C produced is also 0.125 mol.
Finally, we can convert moles of C to mass using the molar mass:
0.125 mol * 12.01 g/mol = 1.50 g
Therefore, the mass of C produced in 10 seconds is approximately 1.50 grams.