Neutron is subatomic particel with with mass approximately one atomic mass unit, and neutron mass slightly larger than proton.
neutron have natural charge and i suppose that the mass may be called as: a. mass number of 1.
hope this help
CO(g) +2H2--->CH3OH
2.50g H2*1mol/2g=1.25 mol H2
30.0L CO*1mol/22.4L=1.34 mol CO,
according to reaction 1 mol CO needs 2 mol H2,so 1.34 mol CO need 2.68 mol H2, so 1) limiting teactant is H2 (H)
2)1.25 mol CH3OH will be produced, 1.25 mol*32g/mol=40.0 g CH3OH
3) 1.25 mol H2 needs 0.625 g CO
1.34-0.625=0.715 g CO leftover
NH4^+ + OH^- ==> NH3 + H2O
<span>Set up an ICE chart. </span>
<span>initial: </span>
<span>NH4^+ = mL x M = 100 x 0.1 = 10 millimoles </span>
<span>NH3 = mL x M = 80 x 0.20 = 16 millimoles. </span>
<span>change: </span>
<span>we add 0.2 g NaOH which is 0.2/40 = 0.005 moles or 5 millimoles. </span>
<span>NH3 = +5 millimoles </span>
<span>NH4^+ = -5 millimoles </span>
<span>equilibrium: </span>
<span>NH3 = 16 + 5 = 21 millimoles. </span>
<span>NH4^+ = 10 - 5 = 5 millimoles. </span>
<span>You may substitute millimoles in place of concn (since millimoles/mL = molarity and the mL (180 mL) appears in both numerator and denominator) OR you can divide millimoles/180 mL to arrive at concn for both base and acid and substitute those numbers. Plug those into the HH equation and solve for pH. </span>
<span>For part d, just set up the HH equation and pH = pKa + log (base/acid). The question is asking you to calculate pH if base and acid were equal. So plug in the same number (any number you choose) for base and acid and calculate. Note that the log of 1 = 0</span>
If the ion has a charger of -1 and 10 electrons then it has 9 protons
Answer: Complete ionic equations dissociate all aqueous solutions into ions. Net ionic equations show the change that occurs in chemical reactions and do not show spectator ions that are the same in reactants and products. (b) If no spectator ions were present then complete and net ionic equations would be identical.
Explanation: