assuming you mean 30gs-3 this means 30 grams per thousandth of a second
3^6 = 729
27 3 to the power of 3 3 x 3 x 3 (3 x 3) x 3 9 x 3 27
2 x 3 x 3 x 3 = 54 2 x 3 x 5 x 7 = 210 2 x 3 x 3 x 3 x 5 x 7 = 1890, the LCM
2 x 2 x 2 x 3 x 3 x 3 = 216 2 x 2 x 2 x 2 x 2 x 3 x 3 = 288 2 x 2 x 2 x 3 x 3 x 5 = 360
2 x 2 x 2 x 2 x 3 x 3 x 3 x 3 x 5 = 6480
20 x 500 mg = 10g or 10g = 500mg x 20
10g/410g X 100 = 2.4 2.5 %
I had to do this problem on a sample exam I got from the University of South Carolina. It has to do with a stoichiometry reaction. If I got the answer wrong, I apologize but this is how I did it. I'll use 2 approaches so you can understand all the concepts going into it. And forget about the "excess H_2" so it doesn't throw you off. First write a balanced equation of the reactants and product: N_2 + 3H_2 -----> 2NH_3 N_2 = 10g 10g of N_2 x [1 mol N_2 / (14.0067x2)] x (3 mol H_2 / 1 mol N_2) x [(1.0079x2) / 1 mol H_2] so, 10 x (1 / 28.0134) x (3) x (2.0158), is 10 x (.03569) x (3) x (2.0158) = 2.158 grams of H_2 Since we have 10g of N_2, we can add the two numbers and find out the mass of ammonia. 10g + 2.158 = 12.158g, or 12 g NH_3. Similarly we can substitute the ammonia (NH_3) for the H_2 in the equation above and get the same answer. 10g of N_2 x [1 mol N_2 / (14.0067x2)] x (2 mol NH_3 / 1 mol N_2) x [(14.0067 + (1.0079 x 3)) / 1 mol NH_3] so, 10 x (1 / 28.0134) x (2) x (17.0304), is 10 x (.03569) x (2) x (17.0304) = 12.158 g, or 12 g NH_3
If you are on 10g or later and the recycle bin feature is turned on, you can use the FLASHBACK TABLE x TO BEFORE DROP command, where x is the name of the table. If it is not there, or the recycle bin feature is not available, you will have to restore the table from a backup.
5(X - 5) + 2g(X - 5)-------------------------------all the factoring I can see
To determine the number of atoms in 10g of Fe, you first need to calculate the number of moles of Fe using its molar mass (55.85 g/mol). Then, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of atoms in those moles of Fe. Finally, multiply the number of moles by Avogadro's number to get the total number of atoms in 10g of Fe.
10G networks transfer at a maximum of 10 gigabits per second.
1 kg = 1000g (kilo=1000)0.01 kg = 0.01 x 1000g = 10g
To calculate the number of moles in 10g of iodine, you need to first determine the molar mass of iodine (I), which is 126.9 g/mol. Then, you can use the formula: moles = mass / molar mass. So, moles = 10g / 126.9 g/mol ≈ 0.079 moles of iodine.
After 2 half-lives (two half-lives of tritium is 12.32 x 2 = 24.64 years), the initial 10g sample of tritium would have decayed by half to 5g.
No, they do NOT contain the same number of particles (either molecules N2 or atoms C): there molecular or atomic mass is different.Look at this:10g N2 / 28 (g/mole N2) x 6.022x1023 (molecules N2/mole N2) = 2.15 x1023 molecules N210g C / 12 (g/mole C) x 6.022x1023 (atoms C/mole C) = 5.02 x1023 atoms C
10 grams nitrogen (1 mole N/14.01 grams)(6.022 X 1023/1 mole N) = 4.3 X 1023 atoms of nitrogen ======================