<span>The correct option is C.i.e. AlCl3
Given:
The valence of aluminum is +3, and the valence of chlorine is –1. Thus, 3 chlorine atoms each of (-1 charge )combine to make the charge balance because of Al (3+). Thus, 1 atom of Aluminum (Al) binds with three atoms of Chlorine (Cl).Thus, the net foromula becomes AlCl3</span>
<span>In the reverse reaction HF is a reactant.</span>
The burning of glucose in presence of oxygen is called as combustion
The balanced reaction is
C6H12O6 + 6O2 ---> 6CO2 + 6H2O
Thus for each mole of glucose we need six moles of oxygen molecules
molar mass of glucose is 180g / mole
The moles of glucose present = mass / molar mass = 180 / 180 = 1 mole
The moles of oxygen present = mass / molar mass = 192 / 32 = 6 moles
Thus the reaction will go to completion and one mole of glucose will react with six moles of O2 to give six moles of CO2 and six moles of H2O
Mass of CO2 produced = moles X molar mass = 6 x 44 = 264 g
Mass of H2O produced = moles X molar mass = 6 x 18 = 108 g
Answer:
5.63 g
Explanation:
Step 1: Write the balanced equation
CuBr₂(aq) + 2 AgCH₃CO₂(aq) ⇒ 2 AgBr(s) + Cu(CH₃CO₂)₂(aq)
Step 2: Calculate the reacting moles of copper (II) bromide
30.0 mL of 0.499 M CuBr₂ react. The reacting moles of CuBr₂ are:
Step 3: Calculate the moles formed of silver (I) bromide
The molar ratio of CuBr₂ to AgBr is 1:2. The moles formed of AgBr are 2/1 × 0.0150 mol = 0.0300 mol.
Step 4: Calculate the mass corresponding to 0.0300 mol of AgBr
The molar mass of AgBr is 187.77 g/mol.
Answer:
False
Explanation:
False. The molecules of liquid are hold in the liquid state due to intermolecular forces or Van de Waals forces , without affecting the molecule itself and its atomic bonds (covalent bonds). When the temperature increases the kinetic energy of the molecules is higher , therefore they have more possibilities to escape from the attractive intermolecular forces and go to the gas state.
Note however that this is caused because the intermolecular forces are really weak compared to covalent bonds, therefore is easier to break the first one first and go to the gas state before any covalent bond breaks ( if it happens).
A temperature increase can increase vaporisation rate if any reaction is triggered that decomposes the liquid into more volatile compounds , but nevertheless, this effect is generally insignificant compared with the effect that temperature has in vaporisation due to Van der Waals forces.
